Deck 3: Compounds

Question 1

Which of the following is a cation?

A) Ca²⁺
B) Na
C) Br
D) O^2-

Answer 1

Ca²⁺

Question 2

Which of the following is an anion?

A) F
B) Al³⁺
C) Mg
D) I^-

Answer 2

I^-

Question 3

CO₃^2- is the ___ ion.

A) acetate
B) hydrogencarbonate (bicarbonate)
C) carbonate
D) cyanide

Answer 3

carbonate

Question 4

The formula of a phosphate ion is ___.

A) PO₄^3-
B) P^3-
C) HPO₄^2-
D) H₂PO₄^-

Question 5

The name for the Cu²⁺ ion is

A) copper ion.
B) cobalt (II) ion.
C) copper (I) ion.
D) copper(II) ion.

Question 6

NO₃^- is the ___ ion.

A) nitrous
B) nitrogen trioxide
C) nitrite
D) nitrate

Question 7

HPO₄^2- is the ___ ion.

A) hydrogen phosphate
B) monophosphate
C) phosphide
D) phosphite

Question 8

Which symbol is representative of a halide ion?

A) He
B) Ne
C) I^-
D) Fe²⁺

Question 9

The name for the Ti⁴⁺ ion is

A) Tin ion.
B) Tin (IV) ion.
C) Titanium ion.
D) Titanium (IV) ion.

Question 10

The formation of ions typically occurs when

A) nonmetal atoms lose electrons and metals gain them.
B) metal and nonmetal atoms are close together in the number of valence electrons.
C) metal and nonmetal atoms have the same number of electrons.
D) nonmetal atoms gain electrons and metal atoms lose them.

Question 11

Which is the appropriate description of Sr²⁺?

A) This is an atom and can be used to form chemical compounds.
B) This is an atom with a charge of +2 because there are more neutrons than protons.
C) This is an ion with a charge of +2 because there are two more protons than electrons.
D) This is an ion with a charge of +2 because there are more electrons than protons.

Question 12

Nitrogen can have an anion, N^3-. This ion

A) is the result of the atom gaining three electrons.
B) can form three ionic bonds.
C) has eight electrons in the outside orbit.
D) All of these choices are correct.

Question 13

How many electrons are contained in sulfide ion?

A) 18
B) 14
C) 30
D) 16

Question 14

Which ion has the same number of electrons as the noble gas argon?

A) F^-
B) Mg²⁺
C) Br^-
D) Ca²⁺

Question 15

Choose the electron dot structure for a magnesium atom.

A)
B)
C)
D)

Question 16

According to the octet rule, how many valence electrons are present in a chloride ion (Cl^-)?

A) 1
B) 2
C) 8
D) 4

Question 17

How many valence electrons must S atom gain to reach an octet?

A) 1
B) 2
C) 3
D) 0

Question 18

According to the octet rule, strontium (Sr) will form which of the following monoatomic ions?

A) Sr^2-
B) Sr³⁺
C) Sr²⁺
D) Sr^3-

Question 19

Generally, the octet rule works fairly well for predicting the behavior of atoms. However, there is an exception:

A) The halogens do not form ions on the basis of the octet rule.
B) The alkali metals only conform to the octet rule when producing neutral atoms.
C) The transition metals do not necessarily conform to the octet rule.
D) The nonmetals do not conform to the octet rule.

Question 20

When considering the octet rule, the explanation of the O^2- ion is

A) a loss of two electrons to get closer to 8 in the energy level.
B) when an oxygen atom gains two electrons, it has the same electron arrangement as neon, an inert gas.
C) oxygen's nuclear charge of 8 can only hold 8 electrons in the outer shell.
D) oxygen is an exception to the octet rule.

Question 21

A compound is

A) two or more elements well mixed.
B) two or more elements combined chemically.
C) two or more elements carrying a positive charge.
D) a physical blend of two or more elements.

Question 22

Which pair of elements cannot combine to form a chemical compound?

A) Na and Ne
B) Li and O
C) Fe and S
D) Ca and I

Question 23

Which of the following atom pairs would most likely be connected by an ionic bond?

A) K and Br
B) O and Br
C) S and Br
D) F and Br

Question 24

Calcium chloride has the formula CaCl₂. As an ionic compound it is

A) composed of one cation and 2 anions.
B) held together by means of covalent bonds.
C) composed of two cations and one anion.
D) more likely a molecular compound.

Question 25

Chose the formula of cobalt(II) nitrate.

A) CoN
B) Co₂ NO₃
C) Co(NO₃)₂
D) Co_(II)(NO₃)₂

Question 26

What is the formula of beryllium sulfide?

A) BeS
B) Be₂S
C) Be₂S₃
D) Be₃S₂

Question 27

What is the proper name of the compound FePO₄?

A) iron phosphide
B) iron(III) phosphide
C) iron(III) phosphate
D) iron phosphorus tetraoxide

Question 28

What is the formula of the ionic compound that forms between lithium ions and dichromate ions?

A) LiCr₂O₇
B) Li₃ Cr₂O₇
C) Li₂ Cr₂O₇
D) Li₄Cr₂O₇

Question 29

The name of the compound Na₂CO₃ is

A) sodium carbonate.
B) disodium carbonate.
C) sodium bicarbonate.
D) disodium bicarbonate.

Question 30

Which of the following is an ionic compound?

A) CS₂
B) CO₂
C) Mg(OH)₂
D) CH₄

Question 31

What is the formula of the ionic compound that forms between calcium ions and phosphate ions?

A) CaPO₄
B) Ca₂PO₄
C) Ca₂(PO₄)₃
D) Ca₃(PO₄)₂

Question 32

The difference between an ionic bond and a covalent bond is that

A) ionic bonds commonly occur between two metals and covalent bonds occur between metals and nonmetals.
B) ionic bonds are between atoms that can share electrons; covalent bonds are between atoms that will donate/accept electrons.
C) covalent bonds come about because of a sharing of electrons; ionic bonds do not.
D) ionic bonds are between smaller atoms; covalent bonds are between large atoms.

Question 33

Predict the number of covalent bonds by S atom.

A) 1
B) 2
C) 3
D) 4

Question 34

Which of the following is a binary compound?

A) NaOH
B) FeCl₃
C) Ca ₃(PO₄)₂
D) None of these choices is a binary compound.

Question 35

The name of the compound N₂O₄ is

A) nitrogen oxide.
B) nitrogen tetroxide.
C) dinitrogen tetroxide.
D) nitrogen dioxide.

Question 36

What is the correct name of the compound Cl₂O₃?

A) dichlorine trioxide
B) Chlorine oxide
C) Chlorine trioxide
D) Chloride oxide

Question 37

What is the molar mass of ammonium oxide?

A) 30.00 g/mol
B) 34.00 g/mol
C) 44.00 g/mol
D) 52.00 g/mol

Question 38

What is the molar mass of isopentyl acetate, C₇H₁₄O₂, a compound responsible for the odor of bananas?

A) 130.19 g/mole
B) 98.32 g/mole
C) 146.58 g/mole
D) 119.35 g/mole
E) 13.19 g/mole

Question 39

What is the molar mass of aspirin (C₉H₈O₄), a drug often used to relieve minor aches and pains?

A) 165.43 g/mol
B) 106.21 g/mol
C) 88.67 g/mol
D) 180.16 g/mol

Question 40

A compound commonly called trisodium phosphate, Na₃PO₄, is used to clean grease and other organic materials from concrete surfaces. Calculate the formula weight of this cleaner.

A) 70.20 amu
B) 116.70 amu
C) 118.30 amu
D) 164.00 amu

Question 41

Aluminum sulfate, Al₂(SO₄)₃, can be used in water purification. What is the formula weight of this salt?

A) 75.10 amu
B) 342.30 amu
C) 315.30 amu
D) 150.10 amu

Question 42

What is the mass in grams of 3 moles of calcium carbonate, CaCO₃, a common antacid?

A) 300 grams
B) 150 grams
C) 100 grams
D) 68 grams

Question 43

Calculate the mass of 10.00 moles of nickel(II) cyanide, Ni(CN)₂.

A) 847.0 grams
B) 987.0 grams
C) 1107 grams
D) 1694 grams

Question 44

Glycerol, often called glycerine, was used as a skin moisturizer before more commercial preparations were made available. Calculate the weight of 7.85 moles glycerin.

A) 92.3 grams
B) 228 grams
C) 667 grams
D) 722 grams

Question 45

Ethanol, C₂H₅OH, is found in alcoholic beverages. If a 125-g sample is pure ethanol, how many moles of ethanol are present?

A) 0.419 moles
B) 2.72 moles
C) 5750 moles
D) 46.3 moles

Question 46

A 1.0 x 10²- gram sample is found to be pure alanine, an amino acid found in proteins. How many moles of alanine are in the sample?

A) 0.20 moles
B) 0.90 moles
C) 1.1 moles
D) 890 moles

Question 47

What is the mass of 0.00142 mole of vitamin C (C₆H₈O₆)?

A) 0.250 g
B) 0.500 g
C) 0.125 g
D) 2.50 g

Question 48

How many molecules of aspirin (C₉H₈O₄) are present in 41.40 g of aspirin?

A) 0.2300 aspirin molecules
B) 2.700 x 10²⁶ aspirin molecules
C) 9.600 x 10²³ aspirin molecules
D) 1.383 x 10²³ aspirin molecules

Question 49

Ag⁺ is an ion with 47 protons and 108 electrons.

Question 50

A Roman numeral is used in the name of transition metal ions. That numeral indicates the charge of the ion.

Question 51

Helium forms an ion with a 2+ charge.

Question 52

SO₃^2- is called the sulfur trioxide ion.

Question 53

Elements in family 8A tend to form anions.

Question 54

Sodium carbonate is an ionic compound whose formula is NaCO₃.

Question 55

The formula of the ionic compound that forms between aluminum ions and Sulfide ions is AlS₂.

Question 56

Potassium and magnesium cannot form a binary compound together.

Question 57

The formula weight of magnesium fluoride is 62.30 amu.

Question 58

The magnesium ___ is represented by Mg²⁺.

Question 59

Roman numerals are used to denote the charge of ___ metal cations if they form more than one ionic charge.

Question 60

The bicarbonate ion is different than the carbonate ion because it contains one ___ not found in the carbonate ion.

Question 61

Ionic compounds tend to exist in the ___ state at room temperature.

Question 62

___ is the formula for aluminum fluoride.

Question 63

The formula of manganese(II) oxide is ___.

Question 64

The valence electrons not involved in bonds are called ___.

Question 65

The oxygen gas found in the atmosphere contains ___ atom(s) per molecule.

Question 66

The risk of heart attack and stroke increase when a person is given blood transfusion because ___ is lacking in stored blood.

Question 67

Complete the following table:

Question 68

Sketch electron dot structures for each of the following atoms:
a) Cl
b) Al
c) Ca
d) N

Question 69

Give the name for each of the following:
a) SiF₄
b) CuBr₂
c) MgCO₃
d) NH₄NO₃

Question 70

Draw the line bond structure of sulfuric acid.

Question 71

Draw a structure expected from the combination of nitrogen and three chlorine atoms?

Question 72

Name the following compounds:
a) MgCl₂
b) AgNO₃
c) Fe(N0₃)₃
d) SCl₂

Question 73

Give the formula for the following compounds:
a) diphosphorus triiodide
b) silver oxide
c) cobalt (II) phosphate
d) carbon disulfide

Question 74

Give the formula for the following compounds:
a) strontium bromide
b) disulfur trioxide
c) copper(II) nitrite
d) lithium oxide

Question 75

Give the name for each of the following:
a) N₂Br₄
b) NH₄Cl
c) Fe(NO₃)₃
d) NaF

Question 76

Determine the molar mass for each of the following:
a) Ca(NO₃)₂
b) AgNO₃
c) FeBr₂
d) SCl₂

Question 77

Calculate the number of moles in 8.61 grams of calcium nitrate.

Question 78

What is the mass in grams of 1.82 x 10^-1 moles of phosphorus trichloride?

Question 79

What is the mass of 3.15 moles of calcium sulfate, CaSO₄?

Question 80

How many moles are in 25.00 g of water?