Deck 3: Molecules, Compounds and Chemical Equations

Question 1

Which of the following is a molecular element?

A)Kr
B)Ag
C)S
D)Mg
E)Ti

Answer 1

S

Question 2

Give the name for SnO.

A)tin (I)oxide
B)tin (II)oxide
C)tin (III)oxide
D)tin (IV)oxide

Answer 2

tin (II)oxide

Question 3

Which of the following is an ionic compound?

A)SCl₂
B)Mg₃(PO₄)₂
C)Cl₂O
D)CH₂O
E)PF₅

Answer 3

Mg₃(PO₄)₂

Question 4

Which of the following is an ionic compound?

A)LiCl
B)NO₂
C)PCl₃
D)CF₄
E)SeBr₂

Question 5

An ionic bond is best described as

A)the sharing of electrons.
B)the transfer of electrons from one atom to another.
C)the attraction that holds the atoms together in a polyatomic ion.
D)the attraction between 2 nonmetal atoms.
E)the attraction between 2 metal atoms.

Question 6

Write the formula for the compound formed between potassium and sulfur.

A)KS
B)KS₂
C)K₂S
D)K₂SO₃
E)K₃S₂

Question 7

Which of the following is a molecular element?

A)Mg
B)Ar
C)Xe
D)I
E)Li

Question 8

Give the name for NaNO₃.

A)sodium nitrite
B)sodium nitrate
C)sodium pernitrate
D)sodium hyponitrite
E)sodium hyponitrate

Question 9

Write a possible molecular formula for C₄H₄O.

A)C₈H₈O₂
B)C₁₂H₁₂O₂
C)C₂H₂O
D)C₈H₈O

Question 10

Which of the following is a molecular compound?

A)CuCl₂
B)KCl
C)NaNO₃
D)CH₃Cl
E)RbBr

Question 11

Which of the following is an atomic element?

A)Br
B)H
C)N
D)O
E)Mg

Question 12

What is the empirical formula for Hg₂(NO₃)₂?

A)Hg₂(NO₃)₂
B)HgNO₃
C)Hg(NO₃)₂
D)Hg₂NO₃
E)Hg₄(NO₃)₄

Question 13

Determine the name for TiCO₃.Remember that titanium forms several ions.

A)titanium (II)carbonate
B)titanium carbide
C)titanium carbonite
D)titanium (II)carbonite
E)titanium (I)carbonate

Question 14

Give the formula for sodium chlorate.

A)NaClO
B)NaClO₂
C)NaClO₃
D)NaClO₄

Question 15

Which of the following is a molecular compound?

A)NaCN
B)LiOH
C)SrI₂
D)ZnS
E)P₄O₁₀

Question 16

Write the formula for barium nitrite.

A)Ba₃N₂
B)BaNO₃
C)BN
D)Ba(NO₂)₂
E)B(NO₂)₃

Question 17

Write the name for Sn(SO₄)₂.Remember that Sn forms several ions.

A)tin (I)sulfite
B)tin (IV)sulfate
C)tin sulfide
D)tin (II)sulfite
E)tin (I)sulfate

Question 18

A covalent bond is best described as

A)the sharing of electrons between atoms.
B)the transfer of electrons.
C)a bond between a metal and a nonmetal.
D)a bond between a metal and a polyatomic ion.
E)a bond between two polyatomic ions.

Question 19

Write the formula for strontium nitride.

A)Sr₃N₂
B)Sr(NO₃)₂
C)SrN
D)Sr₂N₃
E)Sr(NO₂₎₂

Question 20

What is the empirical formula for C₄H₁₀O₂?

A)C₂H₅O
B)CHO
C)C₂H₄O
D)CHO₂
E)CH₂O

Question 21

Calculate the molar mass of Al(C₂H₃O₂)₃.

A)86.03 g/mol
B)204.13 g/mol
C)56.00 g/mol
D)258.09 g/mol
E)139.99 g/mol

Question 22

How many millimoles of Ca(NO₃)₂ contain 4.78 × 10²² formula units of Ca(NO₃)₂? The molar mass of Ca(NO₃)₂ is 164.10 g/mol.

A)12.6 mmol Ca(NO₃)₂
B)13.0 mmol Ca(NO₃)₂
C)20.7 mmol Ca(NO₃)₂
D)79.4 mmol Ca(NO₃)₂
E)57.0 mmol Ca(NO₃)₂

Question 23

Determine the name for CoCl₂^∙6H₂O.Remember that Co forms several ions.

A)cobalt chloride hydrate
B)cobalt (I)chloride heptahydrate
C)cobalt (II)chloride heptahydrate
D)cobalt (II)chloride hexahydrate
E)cobalt (I)chloride

Question 24

Calculate the molar mass for Mg(ClO₄)₂.

A)223.21 g/mol
B)123.76 g/mol
C)119.52 g/mol
D)247.52 g/mol
E)75.76 g/mol

Question 25

Determine the name for P₄O₁₀.

A)phosphorus (IV)oxide
B)diphosphorus pentoxide
C)phosphorus oxide
D)phosphorus (II)oxide
E)tetraphosphorus decoxide

Question 26

Determine the name for H₂CO₃.

A)carbonous acid
B)dihydrogen carbonate
C)carbonic acid
D)hydrocarbonic acid
E)hydrocarbide acid

Question 27

Write the name for Ca₃(PO₄)₂.

A)calcium (III)phosphite
B)calcium (II)phosphite
C)calcium phosphate
D)tricalcium phosphorustetraoxide
E)calcium phosphite

Question 28

Give the correct formula for aluminum sulfate.

A)Al₂2SO₄
B)Al(SO₄)₃
C)Al₃(SO₄)₂
D)Al₂(SO₄)₃

Question 29

Determine the name for Cl₂O.

A)chlorine oxide
B)dichlorine monoxide
C)chlorine (I)oxide
D)chlorine (II)oxide
E)chlorate

Question 30

How many N₂O₄ molecules are contained in 76.3 g N₂O₄? The molar mass of N₂O₄ is 92.02 g/mol.

A)5.54 × 10²⁵ N₂O₄ molecules
B)7.26 × 10²³ N₂O₄ molecules
C)1.38 × 10²⁴ N₂O₄ molecules
D)4.59 × 10²⁵ N₂O₄ molecules
E)4.99 × 10²³ N₂O₄ molecules

Question 31

How many C₂H₄ molecules are contained in 45.8 mg of C₂H₄? The molar mass of C₂H₄ is 28.05 g/mol.

A)9.83 × 10²⁰ C₂H₄ molecules
B)7.74 × 10²⁶ C₂H₄ molecules
C)2.71 × 10²⁰ C₂H₄ molecules
D)3.69 × 10²³ C₂H₄ molecules
E)4.69 × 10²³ C₂H₄ molecules

Question 32

Give the formula for sulfurous acid.

A)H₂SO₃
B)HSO₃
C)H₂SO₄
D)HSO₄

Question 33

Calculate the molar mass of C₈H₆O₄.

A)166.13 g/mol
B)182.09 g/mol
C)150.18 g/mol
D)172.13 g/mol

Question 34

Determine the name for aqueous HBr.

A)bromic acid
B)bromous acid
C)hydrobromous acid
D)hydrogen bromate
E)hydrobromic acid

Question 35

How many moles of C₃H₈ contain 9.25 × 10²⁴ molecules of C₃H₈?

A)65.1 moles C₃H₈
B)28.6 moles C₃H₈
C)34.9 moles C₃H₈
D)46.2 moles C₃H₈
E)15.4 moles C₃H₈

Question 36

Identify the formula for nitric acid.

A)HNO₃
B)HNO₂
C)HNO
D)HNO₄

Question 37

Determine the name for N₂O₅.

A)dinitrogen pentoxide
B)nitrogen oxide
C)nitrogen (IV)oxide
D)nitrogen (II)oxide
E)nitrogen tetroxide

Question 38

Calculate the molar mass of Ca₃(PO₄)₂.

A)87.05 g/mol
B)215.21 g/mol
C)310.18 g/mol
D)279.21 g/mol
E)246.18 g/mol

Question 39

Write the formula for copper (II)sulfate pentahydrate.

A)Cu₂SO₃^∙H₅
B)Cu₂S^∙H₂O
C)CuS^∙5H₂O
D)(CuSO₄)₅
E)CuSO₄^∙5H₂O

Question 40

Determine the name for HClO₃.

A)hydrochloric acid
B)hydrochlorus acid
C)chlorate acid
D)chloric acid
E)perchloric acid

Question 41

Determine the empirical formula for a compound that contains C,H and O.It contains 51.59% C and 35.30% O by mass.

A)C₂H₆O
B)CHO
C)C₄H₁₃O₂
D)CH₄O₃
E)CH₃O

Question 42

What is the mass,in kg,of 6.89 × 10²⁵ molecules of CO₂? The molar mass of CO₂ is 44.01 g/mol.

A)3.85 kg
B)5.04 kg
C)2.60 kg
D)3.03 kg
E)6.39 kg

Question 43

How many moles of N₂O₃ contain 2.55 × 10²⁴ oxygen atoms?

A)1.41 moles N₂O₃
B)4.23 moles N₂O₃
C)12.7 moles N₂O₃
D)7.87 moles N₂O₃
E)2.82 moles N₂O₃

Question 44

Give the mass percent of carbon in C₁₄H₁₉NO₂.

A)38.89%
B)72.07%
C)5.17%
D)2.78%

Question 45

Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an empirical formula of NO₂.

A)N₂O₃
B)N₃O₆
C)N₂O₄
D)NO₂
E)N₂O₅

Question 46

Determine the volume of hexane that contains 5.33 × 10²² molecules of hexane.The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.

A)8.59 mL
B)13.5 mL
C)7.40 mL
D)12.4 mL
E)11.6 mL

Question 47

Two samples of potassium iodide are decomposed into their constituent elements.The first sample produced 13.0 g of potassium and 42.3 g of iodine.If the second sample produced 24.4 kg of potassium,how many kg of iodine were produced?

A)13.3 kg
B)22.5 kg
C)79.4 kg
D)44.4 kg
E)92.4 kg

Question 48

Calculate the mass percent composition of sulfur in Al₂(SO₄)₃.

A)28.12%
B)9.372%
C)42.73%
D)21.38%
E)35.97%

Question 49

How many moles of PCl₃ contain 3.68 × 10²⁵ chlorine atoms?

A)61.1 moles PCl₃
B)20.4 moles PCl₃
C)16.4 moles PCl₃
D)54.5 moles PCl₃
E)49.1 moles PCl₃

Question 50

How many sodium ions are contained in 99.6 mg of Na₂SO₃?
The molar mass of Na₂SO₃ is 126.05 g/mol.

A)1.52 × 10²⁷ sodium ions
B)4.76 × 10²⁰ sodium ions
C)2.10 × 10²¹ sodium ions
D)1.05 × 10²¹ sodium ions
E)9.52 × 10²⁰ sodium ions

Question 51

How many molecules are contained in 25.0 mL of butane? The density of butane is 0.6011 g/mL and the molar mass is 58.12 g/mol.

A)2.59 × 10²³ molecules butane
B)1.46 × 10²⁷ molecules butane
C)6.87 × 10²³ molecules butane
D)1.56 × 10²³ molecules butane
E)7.14 × 10²⁵ molecules butane

Question 52

What is the mass of 9.44 × 10²⁴ molecules of NO₂? The molar mass of NO₂ is 46.01 g/mol.

A)205 g
B)294 g
C)721 g
D)341 g
E)685 g

Question 53

Combustion analysis of 63.8 mg of a C,H and O containing compound produced 145.0 mg of CO₂ and 59.38 mg of H₂O.What is the empirical formula for the compound?

A)C₅H₂O
B)CHO
C)C₃H₆O
D)C₃H₇O
E)C₆HO₃

Question 54

Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an empirical formula of C₂H₅O₂.

A)C₂H₅O₂
B)C₆H₁₅O₆
C)C₃H₇O₃
D)C₄H₁₀O₄
E)C₈H₂₀O₈

Question 55

Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg Cl.

A)P₃Cl
B)PCl
C)PCl₂
D)P₂Cl₃
E)PCl₃

Question 56

How many moles of C₃H₈ contain 4.95 × 10²⁴ hydrogen atoms?

A)8.22 moles C₃H₈
B)6.58 moles C₃H₈
C)1.03 moles C₃H₈
D)9.73 moles C₃H₈
E)3.09 moles C₃H₈

Question 57

Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.

A)NO
B)N₂O
C)NO₂
D)N₂O₃
E)NO₃

Question 58

How many atoms of oxygen are contained in 47.6 g of Al₂(CO₃)₃? The molar mass of Al₂(CO₃)₃ is 233.99 g/mol.

A)1.23 × 10²³ O atoms
B)2.96 × 10²⁴ O atoms
C)2.87 × 10²⁵ O atoms
D)1.10 × 10²⁴ O atoms
E)3.19 × 10²⁴ O atoms

Question 59

Determine the empirical formula for a compound that is 70.79% carbon,8.91% hydrogen,4.59% nitrogen,and 15.72% oxygen.

A)C₁₈H₂₇NO₃
B)C₁₈H₂₇NO₂
C)C₁₇H₂₇NO₃
D)C₁₇H₂₆NO₃

Question 60

Calculate the mass percent composition of lithium in Li₃PO₄.

A)26.75%
B)17.98%
C)30.72%
D)55.27%
E)20.82%

Question 61

Match the following.
iodine

A)I(s)
B)Cl(g)
C)O(g)
D)Cl2(g)
E)Ne2(g)
F)Ne(g)
G)Ca(s)
H)Q₂(g)
I)I2(s)
J)Ca2(s)

Question 62

Give the name for HNO₂.

Question 63

Match the following.
calcium

A)I(s)
B)Cl(g)
C)O(g)
D)Cl2(g)
E)Ne2(g)
F)Ne(g)
G)Ca(s)
H)Q₂(g)
I)I2(s)
J)Ca2(s)

Question 64

Which of the following is one possible form of pentane?

A)CH₃CH₂CH₂CH₂CH₃
B)CH₃CH=CHCH₂CH₃
C)CH₃CH₂CH₂CH₂CH₂CH₃
D)CH₃CH₂CH₂CH₂CH₂NH₂
E)CH₃CH₂-O-CH₂CH₂CH₃

Question 65

Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.

A)H₂SO₄(aq)+ LiOH(aq)→ H₂O(l)+ Li₂SO₄(aq)
B)H₂SO₃(aq)+ 2 LiOH(aq)→ 2 H₂O(l)+ Li₂SO₃(aq)
C)HSO₃(aq)+ LiOH(aq)→ H₂O(l)+ LiSO₃(aq)
D)HSO₄(aq)+ LiOH(aq)→ H₂O(l)+ LiSO₄(aq)
E)H₂S(aq)+ 2 LiOH(aq)→ 2 H₂O(l)+ Li₂S(aq)

Question 66

Match the following.
oxygen

A)I(s)
B)Cl(g)
C)O(g)
D)Cl2(g)
E)Ne2(g)
F)Ne(g)
G)Ca(s)
H)Q₂(g)
I)I2(s)
J)Ca2(s)

Question 67

Can you predict the chemical formula for a covalent compound between nitrogen and oxygen? Explain your answer.

Question 68

Match the following.
chlorine

A)I(s)
B)Cl(g)
C)O(g)
D)Cl2(g)
E)Ne2(g)
F)Ne(g)
G)Ca(s)
H)Q₂(g)
I)I2(s)
J)Ca2(s)

Question 69

Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.

A)Al(C₂H₃O₂)₂(aq)+ (NH₄)₂PO₄(aq)→ AlPO₄(s)+ 2 NH₄C₂H₃O₂(aq)
B)Al(C₂H₃O₂)₂(aq)+ (NH₃)₂PO₄(aq)→ AlPO₄(s)+ 2 NH₃C₂H₃O₂(aq)
C)Al(CO₃)₂(aq)+ (NH₃)₂PO₄(aq)→ AlPO₄(s)+ 2 NH₃CO₃(aq)
D)Al(C₂H₃O₂)₃(aq)+ (NH₄)₃PO₄(aq)→ AlPO₄(s)+ 3 NH₄C₂H₃O₂(aq)
E)Al(CO₂)₃(aq)+ (NH₄)₃PO₃(aq)→ AlPO₃(s)+ 3 NH₄CO₂(aq)

Question 70

List the elements in a hydrocarbon.

Question 71

Describe the difference between a molecular formula and an empirical formula.Give an example.

Question 72

Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form carbon monoxide gas and water vapor.

A)2 C₂H₆(g)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(g)
B)C₂H₆(g)+ 5 O(g)→ 2 CO(g)+ 3 H₂O(g)
C)2 C₂H₆(g)+ 5 O₂(g)→ 4 CO(g)+ 6 H₂O(g)
D)C₂H₆(g)+ 7 O(g)→ 2 CO₂(g)+ 3 H₂O(g)
E)2 CH₃(g)+ 5 O(g)→ 2 CO(g)+ 3 H₂O(g)

Question 73

Describe the difference between ionic and molecular compounds.Give an example of each.

Question 74

Identify the principal component of natural gas.

A)propane
B)ethane
C)n-butane
D)methane
E)n-pentane

Question 75

Balance the following equation.
____ C₁₀H₁₂ + ____ O_{2 →} ____ H₂O + ____ CO₂

Question 76

Describe the difference between an atomic element and a molecular element.

Question 77

In which set do all elements tend to form anions in binary ionic compounds?

A)C,S,Pb
B)K,Fe,Br
C)Li,Na,K
D)N,O,I

Question 78

Match the following.
neon

A)I(s)
B)Cl(g)
C)O(g)
D)Cl2(g)
E)Ne2(g)
F)Ne(g)
G)Ca(s)
H)Q₂(g)
I)I2(s)
J)Ca2(s)

Question 79

How can one compound contain both ionic and covalent bonds? Give an example.

Question 80

Why aren't prefixes used in naming ionic compounds?