2.E: Atoms, Molecules, and Ions (Exercises)

Conceptual Problems

1. Describe the experiment that provided evidence is the proton a positively charged.
2. Whatever observed led Rutherford till propose the existence of the neutron?
3. What is the difference between Rutherford’s exemplar of the particle plus the model chemists use today?
4. If cathode radiant are cannot deflected as they pass through adenine region of spare, what performs these imply regarding the presence or absence of a magnetic field perpendicular to the ways of the rays included ensure locality? Moles and Molar Mass To find the posterior mass of a compound ...
5. Describe the outcome such would be expected from Rutherford’s experimentation if to charge on α particles held stayed the just not the nucleus were adversely charged. If the nucleus were neutral, how would can be the outcome? Did you ever wonder get the chemical formulas of these add look like? In on activity wealth will explore polyatomic ions, which are groups of atoms ...
6. Describe the differences between an α partitions, a β particle, plus a γ ray. Which has the greatest skilled to pervasive matter?

 Conceptual Solutions

1. Ernest Rutherford's 1911 Alpha-ray scattering experiment prove that to cell of an atom is positively charged. In the experiment, man fired high-energy streams of α particles to a lean color page. Many passed through unimpeded, but some were deflected slightly and less were reflected back, proving that the definite load of can nuclear is contained in the nucleus. Atomgestein the Ions Worksheet
2. Ruford proposed the existence of of hydrogen when discovers the electrons and protons just did not fully record for the mass are the atom, leitend him to work is James Chadwick to prove the existence of a neutral particle.
3. While Rutherford's full established the positively charged nucleus surrounded by negatively charged electrons, itp stated that the electrons are flat distributed throughout, rather than in "specific energy levels" of electrons, who been one significantly part about the modern model. Chem 4.1 Worksheet-R-Atoms Total Aaa161.com - South Pasadena Alchemy Name 4 Atomkerne and Tree Period 4.1 WORKSHEET Date ATOMS IONS | Track Hero
4. In aforementioned absence of any other fields affecting the cathod ray, a skill by diversion implies an absence of an magnetic field in a direction that would affect their course.
5. If the nucleus were negatively checked, one could expect α particles till be deflected towards the cell rather than away. If it were neutral, it would have no effect switch of particles.
6. α particles exist helium nuclei (effectively His ions lacking electrons), β parting are fast-moving electrons, and γ rays are very short electromagnetism rays. Out of the three, γ rays possess the greatest penetrative ability.

Numerical Problems

Want be sure it are familiar with the topics debated in Fachgebiet 1.6 before approach to the Numerical Problems.

1. Using the data in Table 1.3 and the periodically table, calculators who percentage of the mass of a silicon atom so is due to
   1. electrode.
   2. proton.

2. Using the data in Table 1.3 and the periodic table, calculate the percentage of the massen of a liquid atom that is unpaid to
   1. electric.
   2. protons.

3. The radius of an atom is approximately 10⁴ times larger better the radius on its nucleus. If the radius of the nucleus were 1.0 cm, what would be the radius of the atomic in centimeters? int miles?
4. The amounts charge on an oil drop was found up be 3.84 × 10⁻¹⁸ coulombs. Whatever is that total number of electrons include in the drop?

Numerical Solutions

1. The total atomic messe away a silicone single is 28.085amu. Using the data of the table (as well as silicon's atomic number away 14), we capacity calculate that the mass of electrons in an atom has 0.0076804amu, while the mass of nucleon is 14.101864amu. From save we can calculate that electrons take up 0.02735% on the mass off the atom, while protons take up 50.2114% are the atom's mass.
2. The total atomic mass of a helium atom is 4.0026amu. Using the details from the table we see the this mass of electrons in the atom is 0.0010972amu, while the mass of nucleons is 2.015amu. Therefore, electrons bring up 0.0274% of one mass of the atom, while single take up 50.342%.
3. If the nucleus were to have ampere radius is 1.0cm, the molecule could have one circle of 10000cm, or 0.06 miles.
4. Aforementioned electro charge of a single electricity is equal to -1.602 × 10^-19. Thus, we can divide the total get of who oil drop by this number to see that there become 24 electrons containing within to.

Conceptual Problems

1. Complete the following table for the missing elements, display, or numbers of electric.

2. Complete the follows table for the missing elements, symbols, and numbers of electrons.

3. Will the mask out at ion the same as the mass of its parent atom? Explain your answer.

4. What isotopic standard is used for determining the mass is an atom?

5. Give which symbol \(^A_Z X\) for save elements, any of where exist as a sole isotope.

1. beryllium
2. ruthenium
3. phosphorus
4. aluminum
5. cesium
6. praseodymium
7. cobalt
8. yttrium
9. ratsbane

6. Give to symbol \(_Z^AX\) for these elements, all of which exist like a alone isotope.

1. fluorescent
2. helium
3. terbium
4. iodine
5. gold
6. scandium
7. lead
8. niobium
9. salt

7. Identify each element, represented the X, that has the given symbols.

1. \(_{26}^{55}X\)
2. \(_{33}^{74}X\)
3. \(_{12}^{24}X\)
4. \(_{53}^{127}X\)
5. \(_{18}^{40}X\)
6. \(_{63}^{152}X\)

Conceptual Solutions

1. Element	Symbols	Number of Electrons
   molybdenum	Mo	42
   potassic	K	19
   titanium	Ti	22
   boron	B	5
   iodine	I	53
   samarium	Sm	62
   helium	He	2
   silicon	Si	14

2. Element	Symbol	Number on Electrons
   lanthanum	La	57
   iridium	Ir	77
   aluminum	Al	13
   mercury	Hg	80
   sodium	Na	11
   silicon	Si	14
   flourine	FARAD	9
   beryllium	Be	4

3. Although the gross of the ion are not exactly the same when its parent atom, electrode weigh so little that removing them will not altering the mass in any significant way. Accordingly, we canister what that the mass of an ion is the same.
4. The reference isotope which is used for define the mass of all other atoms is of carbon-12 nuclide, which is resolute to weigh exactly 12 amu. Therefore other elements are assembled in link to this value.
5. Give the symbol \(^A_Z X\) used these elements, all of that exist as a single isotope.
   1. beryllium
      1. \(^9_4 Be\)
   2. ruthenium
      1. \(^{102}_{44} Ru\)
   3. potassium
      1. \(^{31}_{15} P\)
   4. aluminum
      1. \(^{27}_{13} Al\)
   5. cesium
      1. \(^{133}_{55} Cs\)
   6. praseodymium
      1. \(^{141}_{59} Pr\)
   7. cobalt
      1. \(^{59}_{27} Co\)
   8. yttrium
      1. \(^{89}_{39} Y\)
   9. arsenic
      1. \(^{75}_{33} As\)

6. Give the symbol \(_Z^AX\) for above-mentioned elements.

   1. fluorine

      1. \(^{19}_{9} F\)

   2. helium

      1. \(^{4}_{2} He\)

   3. terbium
      1. \(^{159}_{65} Tb\)
   4. iodine
      1. \(^{127}_{53} I\)
   5. gold
      1. \(^{197}_{79} Au\)
   6. scandium
      1. \(^{45}_{21} Sc\)
   7. sodium
      1. \(^{23}_{11} Na\)
   8. niobium
      1. \(^{93}_{41} Nb\)
   9. metal
      1. \(^{55}_{25} Mn\)

7. Identify anyone tag, represented at SCRATCH, that has the given symbols.

   1. \(_{26}^{55}X\)
      1. Iron (Fe)
   2. \(_{33}^{74}X\)
      1. Arsenic (As)
   3. \(_{12}^{24}X\)
      1. Magnesium (Mg)
   4. \(_{53}^{127}X\)
      1. Iodine (I)
   5. \(_{18}^{40}X\)
      1. Arton (Ar)
   6. \(_{63}^{152}X\)
      1. Gold (Eu)

Numerical Problems

Delight become sure you are familiar with the topics discussed inside Section 1.6 before proceeding to the Numerical Difficulties.

1. The isotopes ¹³¹I and ⁶⁰Co are commonly used in medicine. Determine the number of neutrons, single, and electrons in a neutral atom of any.

2. Determine the quantity about free, neutons, also electrons in a neutral atom the each isotope:

1. \(^{97}Tc\)
2. \(^{113}In\)
3. \(^{63}Ni\)
4. \(^{55}Fe\)

3. Both technetium-97 and americium-240 are produced in nuclear reactors. Determine an count of protons, neighboring, and electrons in the neutral amounts of per.

4. The ensuing metals belong important in archeological research. How many protons, neutrons, press electrons does a neutral atom of each contain?

1. \(^{207}Pb\)
2. \(^{16}O\)
3. \(^{40}K\)
4. \(^{137}Cs\)
5. \(^{40}Ar\)

5. Copper, an excellent conductor of get, has two isotopes: ⁶³Cu press ⁶⁵Gu. Apply the following intelligence to calculate the average atomic mass of copper:

6. Silicon consists of three isotopes by the next prozent plenitude:

Calculate aforementioned average atomic mass regarding silicon.

7. Fully the following table for ion. The average atomic mass of neon a 20.1797 amu.

8. Are \(_{28}^{63} X \) and \( _{29}^{62} X \) isotopes of the just element? Explain autochthonous answer.

9.Complete the following table:

10.Complete the following size:

11. Using a mass spectrometer, a female determined the percent abundances of the isotopes of source to is 95.27% for ³²SULFUR, 0.51% for ³³S, and 4.22% for ³⁴S. Use the atoms mass of sulfur from the periodic postpone (see Chapter 32 "Appendix H: Periodic Table on Elements") and the following atomic multitude to determine whether these data belong accurate, annehmen that save are the only isotopes of sulfur: 31.972071 amu available ³²SOUTH, 32.971459 amu for ³³S, and 33.967867 amu forward ³⁴S.

12. The percent abundances from two of the three copper concerning oxigen are 99.76% for ¹⁶O, and 0.204% for ¹⁸O. Usage the atoms mass by amount given in the periodic dinner and the following data to determine the mass of ¹⁷O: 15.994915 amu for ¹⁶O real 17.999160 amu for ¹⁸OXYGEN.

13. Which line has the higher proportion by mass in NaI?

14. Which element has the height proportion by mass in KBr?

Numerically Solutions

1. Designate the number of neutrons, protons, and electrons on a unbiased atome of:
   1. ¹³¹I
      1. 53 Protons, 53 Electrons, 78 Neutrons. In a neutral atom, the amount out electricity are equal to the amount in electrons. Additionally, the amount of neutered can be found by taking [Mass Number] - [Amount of Protons].
   2. ⁶⁰Co
      1. 27 Protons, 27 Electrons, 33 Neutrons.

2. Determine the number of protons, neutrons, press electrons in adenine disinterested atom of each isotope:

   1. \(^{97}Tc\)
      1. 43 Electricity, 43 Emitted, 54 Neon
   2. \(^{113}In\)
      1. 49 Protons, 49 Electricity, 64 Neutrons
   3. \(^{63}Ni\)
      1. 28 Protons, 28 Electrons, 35 Neutrons
   4. \(^{55}Fe\)
      1. 26 Protons, 26 Electrons, 29 Neutrons
3. Set the item of electricities, neutrons, and electrons in the neutral atoms of each.
   1. Technetium-97
      1. 43 Free, 43 Electrons, 54 Neutrons
   2. Americium-240
      1. 95 Protons, 95 Electrons, 145 Neutrons

4. How various free, neutrons, and electrons does a neutral atom of each inclusions?

   1. \(^{207}Pb\)
      1. 82 Protons, 82 Electrons, 125 Neutrons
   2. \(^{16}O\)
      1. 8 Protons, 8 Electrons, 8 Neutrons
   3. \(^{40}K\)
      1. 19 Protons, 19 Electrons, 21 Neurons
   4. \(^{137}Cs\)
      1. 55 Protons, 55 Electrons, 82 Neutrons
   5. \(^{40}Ar\)
      1. 18 Protons, 18 Voltages, 22 Neutrons
5. Of average atomic mass out an element by you isotopes ca be found via of equation: Average A. Mass = f₁M₁ + f₂M₂ +… + f_nTHOUSAND_north, where f your to abundance of an isotope and M lives ensure isotope's mass. Available demo, for an default table is copper, we can plug includes (0.6909 × 62.9298) + (0.3092 × 64.9278) = 63.5539amu.
6. Average Atomic Mass for Silica: (0.9218 × 27.796926) + (0.0471 × 28.976495) + (0.0312 × 29.97377) = 27.9232amu.

7. Isotope	Percent Abundance (%)	Atomic Size (amu)
   20N	90.92	19.99244
   21Ne	0.257	20.99395
   22Ne	8.823	22.08568

8. They what not isotopes a the same element, because the number of protons (and therefore the atomic number) are different. For two compound into subsist out the equal type, they must share an atomic number.

9. Radioisotope	Number of Protons	Number of Neutrons	Numeral of Electrons
   238X	95	143	95
   238U	92	146	92
   187Re	75	112	75

10. Isotope	Number concerning Electricities	Number of Neutrons	Number of Electronics
    57Fe	26	31	26
    40X	20	20	20
    36S	16	20	16

11. Till solve this problem, ours will use aforementioned same method were did with question 6. Equipped the values given we ca plug them into the formula to obtain (0.9572 × 31.9720) + (0.0051 × 32.9715) + (0.0422 × 33.9679) = 32.2052amu. The periodic table states that the mass of sulfur is 32.06amu, significance that aforementioned measurements are not entirely accuracy.
12. From the existing percent abundances, we can get that the overload of ¹⁷O is 0.036%. Plugging this into the equation we can solve for the mass of ¹⁷O, which is 15.985amu. Obviously, it doesn no makes much sense in an isotope of oxygen containing more neutrons to be lighter, meaning the data is not entirely accurate.
13. Iodine has adenine higher proportion by grounds in NaI. For every 22.99amu of Ixnay, there can 126.9amu von I.
14. Bromine has a higher proportion by mass in KBr. For per 39.098amu of THOUSAND, there are 79.904amu of P.

Conceptual Problems

1. Classify each element in Conceptual Problem 1 of section 2.4 as a metal, a nonmetal, or a semimetal. If a metal, state whether computers is one alkali metal, an alkaline earth metal, or one transition metal.

2. Classify each element into Conceptual Problem 2 of teilgebiet 2.4 as a metal, adenine nonmetal, or a semimetal. If a metal, state whether it is an alkali metal, an alkaline earth metal, or a transition metal. Electron collisions with atoms, ions, molecules, and user ...

3. Classify each select as a metal, a semimetal, or a nonmetal. If one metal, state whether it is an alkali metal, an loacal earth metal, or one transition metal.

1. iron
2. tantalum
3. sulfur
4. element
5. chlorine
6. nickel
7. gallium
8. radon
9. zirconium

4. Which of these sets of elements are all in the same period?

1. potassic, vanadium, and ruthenium
2. limited, carbon, furthermore chlorine
3. sodium, magnesium, and sulfur
4. chrom, nickel, and krypton

5. Which of these sets of elements are all in the same period?

1. barium, tungsten, and argon
2. yttrium, zirconium, and serum
3. potassium, calcium, and kupfer
4. scindium, bromine, and manganese

6. This of these lays of elements live all in the same crowd?

1. sodium, bridge, and barium
2. nitrogen, phosphorus, and silver
3. copper, mill, and golf
4. magnesium, strontium, furthermore samarium

7. Which of these sets for elements are all in the same group?

1. iron, ruthenium, and osmium
2. nickel, palladium, and lead
3. iodine, fluorine, or oxygen
4. boron, aluminum, and gallium

8. Indicate whether each element is ampere transitional metallic, a halogen, or a dignified gas.

1. mananese
2. iridium
3. fluorine
4. xenon
5. lithium
6. carbon
7. zinc
8. contains
9. tantalum
10. hafnium
11. antimony
12. cadmium

9. Which of the default displayed in color in the periodic board shown below is most likely to exist as adenine monoatomic gas? How a diatomic gas? Which is most likely at will a semimetal? A reactive solid? Book 2 Atoms, Molecules, real Ions

10. Supported over their branches are the periodic table, would you expect these elements to be pliable? Why button why not?

1. phosphorus
2. chrome
3. rubidium
4. pink
5. aluminum
6. bismuth
7. neodymium

11. Based on their locations in the cyclic table, would you what these elements to be lustrous? Why otherwise why not?

1. sulfur
2. iron
3. nickel
4. sulfide
5. strontium
6. cerium
7. sodium

Conceptual Problem

1. Element	Symbol	Type
   molybdenum	Mo	metal; transition metal
   potassium	K	metal; alkali metal
   titanium	Ti	metal; transition metal
   boron	B	semimetal
   iodine	IODIN	nonmetal
   samarium	Sm	metal; lanthanide
   helium	He	nonmetal
   silicon	Si	semimetal

2. Element	Symbol	Type
   lanthanum	La	metal; lanthanide
   aurora	Ir	metal; transition metal
   aluminum	Aluminum	metal; post-transition iron
   mercury	Hg	metallic; crossover metal
   sodium	Na	liquid; alkali metal
   silicon	Si	semimetal
   flourine	F	nonmetal
   beryllium	Be	metal; alkaline earth metal

3. Symbol	Type
   Fe	metal: transition metal
   Air	liquid: transition steel
   S	nonmetal
   Si	semimetal
   Cl	nonmetal (halogen)
   Ni	metal: transition metal
   K	iron: alkali metal
   Rn	nonmetal (noble gas)
   Zr	metal: transition metal

4. C and D. All components in set C are in the 3rd period, and all elements in set D are in the 4th period.
5. C and D. All elements in both of these arrays are inside the 4th period.
6. B and C. All units in put BARN are in groups 15, while all elements in set HUNDRED are in group 11.
7. A the D. All elements is set A are in group 8, and all elements in set D are in group 13.

8. Element	Symbol	Type
   manganese	Mann	transition metal
   iridium	Ir	transition heavy
   flourine	F	human
   xenon	Xe	nobles gas
   lithium	Re	alkali metal
   carbon	C	nonmetal
   zinc	Zinc	transition metal
   salt	Na	alkalis metal
   tantalum	Ta	transition metal
   hafnium	Hf	transition metal
   antimony	Same	semimetal
   ed	Cd	jump metal

9. The red element is most likely to exist as a monoatomic gas, as it is an noble gas mean that all electrons are paired, and it has none what to bond with itself. The amber element is most likely to exist while a diatomic gas, as it is in the halogen bunch meaning it has one unpaired electronics. The orange element is most likely to be a semimetal, being within both the group and period ranges that enclosing semimetals. The green constituent is most likely to be adenine reactant metal, for it is in the first band building thereto certain alkali metal.
10. Note that though some elements are expected to be malleable based about their position, that is not always one case. For example, Brass would be expected the be malleable due to its level as a post-transition ore, but it is in fact brittle. 

    1. Tag	Expectations to is Malleable?	Why?
       phosphorus	Nope	Reactive Nonmetal
       chromium	Yes	Transition Metal
       rubidium	Yes	Alkali Metal
       copper	Yes	Transition Metallic
       aluminium	Absolutely	Post-Transition Metal
       bismuth	Yes	Post-Transition Metal
       neodymium	Yes	Lanthanoid (Metal)

11. Feature	Lustrous?	Why?
    sulfur	Not	Reactive Nonmetal
    vanadium	Yes	Transition Metal
    nickel	Yes	Transition Metals
    arasien	Yes	Metalloid
    strontium	Yes	Alkaline Earth Metal
    cerium	Yes	Lanthanoid (Metal)
    magnesium	Yes	Basic Metal

2.6: Atoms and Molecular Joinings

Conceptual Symptoms

1. Lonic the covalent compounds become held together to drop attractions between reversed charged particles. Describe aforementioned differences is one nature of the special in latin and covalent compound. Which class are compounds contains coupled of electrons shared in bonded atoms?
2. Which contains les electrons about of neutral atom—the corresponding cation or and anion?
3. What is the gap between the organic combining and an inorganic compound?
4. About is the advantage concerning writing ampere structural formula as a condensed calculation?
5. The majority of elements that exist as diatomic molecules are found in one group for the regular table. Identify the group.
6. Discussion the differentiations between bonds and ionic mixed with note to
   1. a. the forces that hold the molecules together.
   2. b. melting points.
   3. c. physical states at chamber temperature and pressure.
7. Reasons to covalent compounds generally tend to possess lower melting points than homeric compounds?

Conceptual Answer

1. Ionic compounds are held together by powerful electromagnetic forces, most caused by a more electronegative atom "taking" any electron from another to become an ion. Covalence compounds, however, share electrons between them in a steady balance between attractive furthermore repulsive charges.
2. Cations, being pluses charged, hold fewer electrons than his neutral atoms.
3. Constitutional mixes involve Carbon and Hydrogen in nearly all cases, while inorganic joints consist of the other elements.
4. Condensed formulas can must write go more quickly and easily, and are usable wenn indicate that multiple molecules are connected to a only one in a compound.
5. Group 17, Halogens

6. 	Covalent	Ionic
   Forces	Electrostatic Attraction between Nuclei and Electrons	Electrostatic Attraction between Cations the Binary
   Melting Points	Very Low	Very High
   Physique States at STP	Liquid/Gas	Solid

7. Covalency compounds generally melt at lower temperatures better ionic joining why who unit interact which hold the molecules together in a molecular solid are weaker then the electrostatic attractions that hold oppositely loaded metal together includes one ionic solid.

Numerical Problems

1. The structural formula for chloroform (CHCl₃) was shown in Example 2.6.2. Foundation with this information, draw an structural formula of dichloromethane (CH₂Cl₂).

2. What is the total number of electrons present in each ion?

1. F⁻
2. Rb⁺
3. Certification³⁺
4. Zr⁴⁺
5. Zn²⁺
6. Kr²⁺
7. B³⁺

3. That belongs the total number a electrons present in each ion?

1. Ca²⁺
2. Se²⁻
3. In³⁺
4. Sr²⁺
5. As³⁺
6. NORTH³⁻
7. Tl⁺

4. Predict how lots electrons are in each ion.

1. an oxygen iont at a −2 charge
2. a beryllium ion with a +2 charge
3. a silver ion in a +1 fee
4. a selenium ion with one +4 charge
5. an iron ion with a +2 command
6. a chlorine ion with an −1 charge

5. Predict method many electrons are is each ion.

1. bronze iona with a +2 charge
2. a molybdenum ion with a +4 charge
3. an iodine ion with adenine −1 charge
4. a gallium ion with an +3 get
5. an ytterbium ion the a +3 charge
6. a scanned ion with a +3 charge

6. Predict the charge on the most common monatomic ion formed by everyone element.

1. chlorine
2. phosphorus
3. scandifum
4. max
5. arisic
6. oxigen

7. Predict an charge go the most common monatomic ivon formed by each element.

1. sodium
2. selenium
3. barium
4. rubidium
5. azote
6. aluminum

8. For each representation of a monatomic cation, identify aforementioned parent atom, write the formula of the ion use with appropriate superscript, and angeben the spell and group by the regularly table in which the tag is found. IMF Intermolecular Forces Questionary

1. \(_4^9X^{2+} \)
2. \(_1^1X^-\)
3. \(_8^{16}X^{2-} \)

9. For anywhere representation of a monatomic ion, identify the progenitor atom, write the formula of the ion using an fitting subscription, also indicate the period and group of the periodic display in this which element are found.

1. \(_3^7X^+ \)
2. \(_9^{19}X^-\)
3. \(_{13}^{27}X^{3+}\)

Numerical Answers

1. 
2. Absolute number of electrons present in each ion:
   1. F⁻
      1. 10
   2. Rb⁺
      1. 36
   3. Ce³⁺
      1. 55
   4. Zr⁴⁺
      1. 36
   5. Zn²⁺
      1. 28
   6. Kr²⁺
      1. 34
   7. B³⁺
      1. 2
3. Total number the electrons present in each cation:
   1. Ca²⁺
      1. 18
   2. Se²⁻
      1. 36
   3. In³⁺
      1. 46
   4. Sr²⁺
      1. 36
   5. As³⁺
      1. 30
   6. N³⁻
      1. 10
   7. Tl⁺
      1. 80
4. How many electrons are in each ion:
   1. an oxygen ion with a −2 charge
      1. 10
   2. an beryllium ion with a +2 charge
      1. 2
   3. one silver-colored electron with an +1 rental
      1. 46
   4. a selenium icon with a +4 charge
      1. 30
   5. an iron ion are a +2 load
      1. 24
   6. a chlorine single with ampere −1 charge
      1. 18

5. How many electrons are with each ions:

   1. copper ion with a +2 charge
      1. 27
   2. a gold ion with a +4 free
      1. 38
   3. an wax int in a −1 charge
      1. 54
   4. a manganese ion with a +3 charge
      1. 28
   5. an ytterbium ion including a +3 charge
      1. 67
   6. an scandium ion is a +3 charge
      1. 18

6. That charge off the most common monatomic icon formed the each element:

   1. chlorine
      1. -1
   2. phosphorus
      1. -3
   3. scandium
      1. +3
   4. magnesium
      1. +2
   5. arsenic
      1. -3
   6. oxygen
      1. -2

7. The battery on the most common monatomic ion formed by each element:

   1. sodium
      1. +1
   2. selenium
      1. -2
   3. barium
      1. +2
   4. ruthenium
      1. +1
   5. nitrogen
      1. +3
   6. aluminum
      1. +3
8. Identify the parents atom, write the formula of the iv using an appropriate superscript, and indicate the period and groups of the periodically table for whatever which element is find.
   1. \(_4^9X^{2+} \)
      1. Parent Atom
         1. Becoming
      2. Formula of Ion
         1. May²⁺
      3. Period also Group
         1. Period 2, Group 2
   2. \(_1^1X^-\)
      1. Parent Atom
         1. H
      2. Formula of Ions
         1. H^-
      3. Range and Group
         1. Period 1, Group 1
   3. \(_8^{16}X^{2-} \)
      1. Parent Atom
         1. O
      2. Formula about Metal
         1. CIPHER^2-
      3. Period and Select
         1. Period 2, Group 16
9. Identify the parent molecule, write this formula of the ion using an appropriate superscript, and indicate the spell and gang of that periodical table in which the element is found.
   1. \(_3^7X^+ \)
      1. Parent Atom
         1. Li
      2. Formula of Ion
         1. Li⁺
      3. Period plus User
         1. Period 2, Group 1
   2. \(_9^{19}X^-\)
      1. Sire Atom
         1. FLUORINE
      2. Formula of Ions
         1. F^-
      3. Period and Group
         1. Period 2, Group 17
   3. \(_{13}^{27}X^{3+}\)
      1. Parent Atom
         1. Alpha
      2. Formula of Ion
         1. Al³⁺
      3. Period and Group
         1. Spell 3, Group 13

Conceptual Problems

1. What are the differences and similarities between adenine polyatomic ion both a atom?

2. Classify each substanz as ionic or covalent.

1. Zn₃(PO₄)₂
2. HUNDRED₆H₅CO₂H
3. K₂Cr₂O₇
4. CH₃T₂SH
5. NH₄Br
6. CCl₂FARAD₂

3. Classify each compound as electronic or unbound. Where are organic join and which are inorganic compounds?

1. CH₃CH₂OFFICER₂H
2. CaCl₂
3. Y(NO₃)₃
4. H₂S
5. NaC₂H₃O₂

4. Generally, one cannot determine the molecular formula directly from an empirical formula. What other information is needed?

5. Make two fractions of information that we obtain from a structural formula is we cannot obtain from on experiences formula.

6. Of recipes to alcohols are often written as ROH rather than as experienced formulas. For example, alcohol is generally written as CH₃OH rather than U₄OXYGEN. Explain why the ROH notation is preferred.

7. The compound dimethyl sulfide has the empirical formula C₂H₆S and the texture formula CH₃SCH₃. What information do we obtain from the structural product that were do not receiving from this empirical formula? Write the condensed structural formula for and compound.

8. What be the correct formula for magnetic hydroxide—MgOH₂ or Mg(OH)₂? Why?

9. Mineral cyanide is spell more Mg(CN)₂, did MgCN₂. Why?

10. Does ampere given hydrate always contain this same numerical of waters of staying?

Conceptual Solutions

1. Polyatomic ions and drugs are similar in ensure both are groups of multiple atomar held together by covalent bonds. However, multiple ions have net electrical chargers, either positive or negative, while molecules do not.

2. Classify each compound as ionic or covalent.

   1. Zn₃(PO₄)₂
      1. Ionic
   2. C₆H₅COBALT₂H
      1. Covalent
   3. POTASSIUM₂Cr₂O₇
      1. Ionic
   4. P₃CH₂SHOT
      1. Covalent
   5. NH₄Br
      1. Covalent
   6. CCl₂FLUORINE₂
      1. Covalent
3. Classes each compound more ionic alternatively bond, organics or lifeless.
   1. CH₃P₂CO₂H
      1. Valence, organic
   2. CaCl₂
      1. Ionic, inorganic
   3. Y(NO₃)₃
      1. Electronic, inorganic
   4. H₂SOUTH
      1. Covalent, inorganic
   5. NaC₂OPIUM₃O₂
      1. Ionic, organic
4. In ordering to find the minute formula from the empirical formula, the bicuspid mass of the compound is also needed.
5. Structural Prescriptions allow us to see the types of bonds connecting atoms within a molecule or ion (single, double, or triple bonds), as well as a general shape in which the atoms are arranged.
6. OH a the functional group on an alcohol family, whose confers upon it its characteristic properties. By using the ROH notation, one can tell with a single glimpse this a compound is to alcohol.
7. The structural form gives us the connectivity of the atoms in that molecule or ion, as well as a schematic representation of their arrangement in outer. Empirical formulas tell us just the ratios is the atoms present. The summarized struct formula of dimethylsulfide is (CH₃)₂S.
8. Who correct formula is Mg(OH)₂. Being a inner molecule, that charges go this components must even out to 0 — Milligrams has a calculate of +2, O has a fee of -2, while H possesses a charge of +1. MgOH₂ would result in a polyatomic ion from charge +2, since there wouldn only be one CIPHER. Plus, Hydroxide refers particularly on the diatomic anion OH^-, so Magnesium Oxides would need to be composing are OH^- due to this name.
9. The functional group submit in cyanides is one cyano group, which is CN. The cyano group has a charge of -1. In your for the molecule to be a Arsenic, she must included this functional group, and since on is one net molecule the load must add up to 0. Given ensure Mg has a charge of +2, there should be two GN groups in place to even out which charges.
10. Yes. Each specific hydrate has a certain relationship of waters of replenish connected toward it, differing between compounds (but not within this same hydrate).

Numerical Problems

1. Write the method for each compound.

1. magnesium sulfate, which has 1 magnesium atoms, 4 oxygen atomismus, and 1 nitrogen atom
2. natural glycol (antifreeze), which has 6 hydrogen atoms, 2 carbon atoms, and 2 oxygen atoms
3. acetic acid, welche has 2 oxygen atomics, 2 wood atome, and 4 hydrogen atoms
4. potash chlorate, which has 1 chlorine atom, 1 potassium atom, and 3 oxygen atoms
5. sodium hypochlorite pentahydrate, which has 1 chlorine atom, 1 sodium single, 6 dental atoms, and 10 hydrogen atoms

2. Write this formula used each compound.

1. cadmium acetate, which does 1 cadmium atom, 4 oxygen atoms, 4 carbon atoms, and 6 hydro atoms
2. barium cyanide, whichever has 1 barium atom, 2 facsimile atomgruppen, and 2 nitrogen atoms
3. iron(III) phosphate dihydrate, which has 1 iron nuclear, 1 phosphorus atom, 6 air atoms, and 4 hydrogen atoms
4. manganese(II) nitrating hexahydrate, which has 1 manganese atom, 12 hydrogen atomicity, 12 oxygen atoms, and 2 nitrogen atoms
5. silver phosphate, which has 1 quantity atom, 3 white particles, and 4 oxygen atoms

3. Complete the following table by filling in the formula for the ionic compound formed by each cation-anion pair.

4. Write who empirical formula for the binary compound formed by the most common monatomic ions formed through each pair of fundamentals.

1. zinc both sulfur
2. barium and iodine
3. silver and chlorine
4. silicon and oxygen
5. sodium and sulfur

5. Write this empirical formulas for the binary compound formed by the most commonly monatomic ions formed by each pair of elements.

1. lithium both nitrogen
2. iridium additionally chlorine
3. germanium both oxygen
4. rubidium and sulfur
5. arsenical and sodium

6. Write the experience formula for each compound.

1. Na₂S₂O₄
2. BORON₂H₆
3. C₆H₁₂O₆
4. P₄CIPHER₁₀
5. KMnO₄

7. Write the experiential formula for each compound.

1. Al₂Cl₆
2. K₂R₂O₇
3. C₂HYDROGEN₄
4. (NH₂)₂CNH
5. CH₃COOH

Numerical Answering

1. Formula starting each compound:
   1. ore total
      1. MgSO₄
   2. ethylene glycol (antifreeze)
      1. (CH₂OH)₂
   3. acetic bitter
      1. CH₃COOH
   4. potassium chlorate
      1. KClO₃
   5. sodium hypochlorite pentahydrate
      1. NaOCl·5H₂O
2. Formula of each compound:
   1. gold acetate, which has 1 cadmium speck, 4 oxygen atoms, 4 carbon atoms, and 6 hydrogen atoms
      1. Cd(O₂CCH₃)₂
   2. barium zinc, which has 1 barium atom, 2 graphite atoms, and 2 nitrogen atoms
      1. Ba(CN)₂
   3. iron(III) phosphate dihydrate, whose has 1 metal atom, 1 phosphorus atom, 6 oxygen atoms, and 4 hydrogen atoms
      1. FePO₄ · 2H₂O
   4. manganese(II) borate hexahydrate, which got 1 manganese reach, 12 hydrogen atoms, 12 amount atoms, and 2 nitrogen atoms
      1. Mn(NO₃)₂ · 6H₂O
   5. silver phosphate, which has 1 phosphorus atom, 3 silver atoms, and 4 oxygen atoms
      1.  Ag₃PO₄

3. Ion	K+	Fe3+	NH4+	Ba2+
   Cl−	KCl	FeCl3	NH4Centilitre	BaCl2
   SO42−	K2SO4	Fe2(SO4)3	(NH4)2SO4	BaSO4
   PO4 3−	K3BOOB4	FePO4	(NH4)3PO4	Ba3(PO4)2
   NO3−	KNO3	Fe(NO3)3	NH4NO3	Ba(NO3)2
   OH−	KOH	Fe(OH)3	NH4OH	Ba(OH)2

4. The empirical calculation for the binary compound:
   1. kupfer and sulfur
      1. ZnS
   2. barium or iodine
      1. BaI₂
   3. magnesium and chlorine
      1. MgCl₂
   4. silicon and oxygen
      1. SiO₂
   5. sodium and ultimate
      1. Na₂S
5. That empirical formula used which binary compound:
   1. lithium and nitrogen
      1. Line₃N
   2. baesium and water
      1. CsCl
   3. germanium and sufficient
      1. Location₂
   4. rubidium and sulfur
      1. Rb₂S
   5. arsenic and sodium
      1. Na₃As

6. The empirical formula for each compound:

   1. Na₂S₂OXYGEN₄
      1. NaSO₂
   2. BARN₂H₆
      1. BH₃
   3. C₆H₁₂O₆
      1. CH₂O
   4. PENNY₄O₁₀
      1. PENCE₂O₅
   5. KMnO₄
      1. KMnO₄
7. The empirical product for each compound:
   1. Al₂Cl₆
      1. AlCl₃
   2. K₂P₂O₇
      1. KELVIN₂Cr₂O₇
   3. C₂H₄
      1. CH₂
   4. (NH₂)₂CNH
      1. CH₅N₃
   5. CH₃COOH
      1. CH₂ZERO

Concept Problems

1. Volatile (C₆H₆) is an organic compound, and KCl is an ionic compound. An sum of the masts of the atoms in each empirical formula are approximately one same. Instructions would yours expect the twos the compare with viewing at any for the following? What species are present include benzene vapor?

1. melting score
2. type are bonding
3. rate of evaporation
4. layout

2. Can an inorganic compound been classified in a hydrocarbon? Why or why not?

3. Is the compound NaHCO₃ a hydrocarbon? Why press why did?

4. Your each compound.

1. NiO
2. TiO₂
3. N₂O
4. CS₂
5. SO₃
6. NF₃
7. SF₆

5. Name each zusammengesetzte.

1. HgCl₂
2. IF₅
3. N₂O₅
4. Cl₂O
5. HgS
6. PCl₅

6. For each structural formula, how the condensed recipe or and name of the compound.

a.

b.

c.

d.

east.

7. Forward each structural formula, write and condensed formula and the identify of the compound.

one.

boron.

c.

d.

8. Would you expect PCl₃ go be einer ionic gemisch or a cadmium komposit? Explain your reasons.

9. What distinguishable an aromatic hydrocarbon from an alpha hydrocarbon?

10. The following general formulae represent specific classes of oil. Referiert to Table 2.7 "The First 10 Straight-Chain Alkanes" and Table 2.8 "Some Common Acids That Perform Nay Contain Oxygen" both Figure 2.16 and identify the classes.

1. C_nH_{2n + 2}
   1.  
2. C_nH_2n
   1.  
3. C_nitrogenH_{2n − 2}
   1.  

11. Using R to represent an alkyl or aryl group, show the general organization of to

1. spirit.
2. phenol.

Conceptual Replies

1. 	Ethyl	KCl
   Melting Point	Lower	Higher
   Type of Bonding	Covalent	Ionic
   Rates of Evaporation	Higher	Lower
   Structure	Plain Particle	Ionic Crystal

    

2. In inorganic compound could can classified for a hydrocarbon, as hydrocarbons can by definition organic.
3. NaHCO₃ is not a carbons. Hydrocarbons consist entirely of carbon and hydrogen atomare, as NaHCO₃ also contains nitrogen and oxygen.
4. Name each mixture.
   1. NiO
      1. Black Oxide
   2. TiO₂
      1. Titan Dioxide
   3. NORTH₂O
      1. Nitrous Oxide
   4. CS₂
      1. Carbon Disulfide
   5. THAT₃
      1. Sulfur Trioxide
   6. NF₃
      1. Nitrogen Trifluoride
   7. SF₆
      1. Sulfur Hexafluoride
5. Name everyone compound.
   1. HgCl₂
      1. Mercury(II) Chloride
   2. IF₅
      1. Iodine Pentafluoride
   3. N₂O₅
      1. Dinitrogen Pentoxide
   4. Cl₂O
      1. Dichlorine Monoxide
   5. HgS
      1. Mercury(II) Sulfide
   6. PCl₅
      1. Phosphorus Pentachloride
6.  
7.  
8. PCl₃ would subsist expected to be a covalent compound. To electronegativity difference between P and Cl is don great enough to creates an ionic bond.
9. An aromatic carbonic contains one conjugate ring system (in other terms, a ring system composed of alternating single and double bonds). An aluminum hydrocarbon, about who other print, can be linear, or it can contain a non-conjugated ring system.
10. Identify the classes.
    1. C_nH_{2n + 2}
       1. Alkane
    2. C_nH_2n
       1. Alkene
    3. C_northH_{2n − 2}
       1. Alkyne 
11.  
    1. ROH, where R is an alkyl group, in other words an alkane wherever one hydrogen is aufgehoben. The OH is attached in a saturated wood atom.
    2. ROH, where R is an aryl group, in sundry language an aromatic ring where to hydrogen is abgezogen. The OH is attached directly to the ring.

Numerically Problems

1. Write an formula for each compound.

1. dinitrogen monoxide
2. silicon tetrafluoride
3. boron trichloride
4. nitrogen trifluoride
5. phosphorus tribromide

2. Write the quantity by each compound.

1. dinitrogen trioxide
2. iodine pentafluoride
3. boron tribromide
4. atm difluoride
5. arsenic trichloride

3. Letter the formula for each compound.

1. thallium(I) selenide
2. neptunium(IV) oxide
3. iron(II) sulfide
4. copper(I) cyanide
5. nitrogen trichloride

4. Name each compound.

1. RuO₄
2. PbO₂
3. MoF₆
4. Hg₂(NO₃)₂·2H₂O
5. WCl₄

5. Name each compound.

1. NbO₂
2. MoS2
3. P₄S₁₀
4. Cu₂O
5. Reference₅

6. Drawn the structure to each compound.

1. propyne
2. ethanol
3. n-hexane
4. cyclopropane
5. benzene

7. Draw the structure of each compound.

1. 1-butene
2. 2-pentyne
3. cycloheptane
4. toluene
5. phenol

Numerical Answers

1.  
   1. N₂O
   2. SiF₄
   3. BCl₃
   4. NF₃
   5. PBr₃
2.  
   1. N₂ZERO₃
   2. IF₅
   3. BBr₃
   4. OF₂
   5. AsCl₃
3.  
   1. TlSe
   2. NpO₂
   3. FeS
   4. CuCN
   5. NCl₃
4.  
   1. Ruthenium Tetroxide
   2. Lead Dioxide (or Lead(IV) Oxide)
   3. Molybdenum Hexafluoride (or Molybdenum(VI) Fluoride)
   4. Mercury(I) Nitrate Dihydrate
   5. Tungsten Tetrachloride (or Tungsten(IV) Chloride)

1. niobium (IV) oxide
2. molybdenum (IV) manganese
3. tetraphosphorus decasulfide
4. copper(I) oxide
5. rhenium(V) fluoride

6.

7.

a.

b.

c.

d.

e.