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Chemistry 4: Lecture 13 Exam Prep

Total questions: 78

Worksheet time: 52mins

Name
Class
Date
1.

Which of the following are properties of protons, neutrons, and electrons?

a)

Protons are positively charged, neutrons have no charge, and electrons are negatively charged.

b)

Protons are negatively charged, neutrons are positively charged, and electrons have no charge.

c)

Protons have no charge, neutrons are negatively charged, and electrons are positively charged.

d)

Protons are negatively charged, neutrons have no charge, and electrons are positively charged.

2.

Elements are classified based on the number of protons as:

a)

Isotopes

b)

Ions

c)

Elements

d)

Molecules

3.

The structure and significance of the Periodic Table can be described as:

a)

A tabular arrangement of elements in order of increasing atomic number, highlighting periodic trends.

b)

A random assortment of elements with no particular order or significance.

c)

A chart that only includes metals and excludes non-metals.

d)

A list of elements organized by their discovery date.

4.

Ions are formed when an atom or molecule gains or loses what?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Photons

5.

Isotopes are atoms of the same element that have different numbers of what?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Nuclei

6.

The average atomic mass of an element is calculated by:

a)

adding the masses of all isotopes

b)

multiplying the mass of each isotope by its natural abundance and summing the products

c)

dividing the total mass by the number of isotopes

d)

using the mass of the most abundant isotope

7.

What are the concepts covered in Chapter 3: 3.1 — 3.7?

a)

Concepts include A, B, and C

b)

Concepts include D, E, and F

c)

Concepts include G, H, and I

d)

Concepts include J, K, and L

8.

List the topics covered in Chapter 4: 4.1 — 4.9.

a)

4.1 — 4.5

b)

4.1 — 4.6

c)

4.1 — 4.7

d)

4.1 — 4.9

9.

What topics are included in Chapter 2: 2.1 — 2.11?

a)

Introduction to basic concepts

b)

Advanced theories and applications

c)

Case studies and examples

d)

Summary and conclusions

10.

How many total questions are there in the exam?

a)

10

b)

20

c)

30

d)

40

11.

What is the point value for each of the 25 main questions in the exam?

a)

1 point

b)

2 points

c)

3 points

d)

4 points

12.

How many bonus questions are included in the exam?

a)

1

b)

2

c)

3

d)

4

13.

What should you bring to the exam?

a)

A pen and a calculator

b)

A laptop and a smartphone

c)

A textbook and notes

d)

A snack and a drink

14.

What is the chemical symbol for Hydrogen?

a)

H

b)

He

c)

O

d)

N

15.

Which group does the element Lithium belong to?

a)

Lithium belongs to Group 1 of the periodic table, also known as the alkali metals.

b)

Lithium belongs to Group 2 of the periodic table, also known as the alkaline earth metals.

c)

Lithium belongs to Group 17 of the periodic table, also known as the halogens.

d)

Lithium belongs to Group 18 of the periodic table, also known as the noble gases.

16.

Identify the category of elements that includes Boron, Carbon, and Nitrogen.

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Noble gases

17.

What is the atomic number of Helium?

a)

1

b)

2

c)

3

d)

4

18.

Which of the following elements is a noble gas?

a)

Oxygen

b)

Neon

c)

Sodium

d)

Iron

19.

What is the general rule for writing chemical formulas with elements?

4 lines
20.

In the chemical formula H2O, what does the subscript '2' indicate?

a)

The subscript '2' in the chemical formula H2O indicates that there are two hydrogen atoms in each molecule of water.

b)

The subscript '2' indicates that there are two oxygen atoms in each molecule of water.

c)

The subscript '2' indicates that there are two molecules of water.

d)

The subscript '2' indicates that there are two atoms of hydrogen and oxygen combined.

21.

What does the implied subscript '1' in H2O indicate?

a)

It indicates there is one oxygen atom in the molecule.

b)

It indicates there is one hydrogen atom in the molecule.

c)

It indicates the molecule is in a gaseous state.

d)

It indicates the molecule is in a liquid state.

22.

How are groups of atoms that act as a unit represented in chemical formulas?

4 lines
23.

What is the basic unit of atomic elements?

a)

Molecules

b)

Single atoms

c)

Compounds

d)

Ions

24.

How many total molecular elements are there to memorize?

a)

5

b)

6

c)

7

d)

8

25.

Ionic compounds are generally composed of _______.

a)

metal + nonmetal

b)

nonmetal + nonmetal

c)

metal + metal

d)

noble gas + metal

26.

Molecular compounds are formed from two or more _______.

a)

nonmetals

b)

metals

c)

metalloids

d)

noble gases

27.

What type of bond is typically found in molecular compounds?

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

28.

How do we write formulas for Ionic Compounds?

a)

By balancing the charges of the ions

b)

By using the periodic table

c)

By guessing the formula

d)

By using molecular geometry

29.

Write a formula for the compound that forms from strontium and chlorine using the following steps: 1. Write the symbol for the metal and its charge followed by the symbol of the nonmetal and its charge. 2. Make the magnitude of the charge on each ion (without the sign) become the subscript for the opposite ion. 3. If possible, reduce the subscripts to give a ratio with the smallest whole numbers. 4. Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the anions.

a)

SrCl

b)

SrCl2

c)

Sr2Cl

d)

Sr2Cl3

30.

Write the symbol for the metal and its charge followed by the symbol of the nonmetal and its charge. [Use Table 5.1 if 2 nonmetals]

a)

Na+ Cl-

b)

K+ Br-

c)

Ca2+ O2-

d)

Mg2+ S2-

31.

Make the magnitude of the charge on each ion (without the sign) become the subscript for the opposite ion.

a)

Use the charge of the first ion as the subscript for the second ion and vice versa.

b)

Use the charge of the second ion as the subscript for the first ion only.

c)

Ignore the charges and use arbitrary subscripts.

d)

Use the charges as they are without changing them.

32.

What is the reduced formula for Barium and Oxygen?

a)

BaO

b)

Ba2O

c)

BaO2

d)

Ba2O3

33.

Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the anions. What is the overall charge?

a)

0

b)

1

c)

-1

d)

2

34.

What is the first step in writing the formula for the compound that forms from sodium and sulfur?

4 lines
35.

What should be done with the magnitude of the charge on each ion when writing the formula for an ionic compound?

4 lines
36.

If possible, reduce the subscripts to give a ratio with the smallest whole numbers. True or False?

a)

True

b)

False

37.

Fill in the blank: Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the _______.

a)

anions

b)

cations

c)

neutrons

d)

protons

38.

Write the symbol for the metal and its charge followed by the symbol of the nonmetal and its charge. [Use Table 5.1 if 2 nonmetals]

a)

Na+ Cl-

b)

K+ Br-

c)

Ca2+ O2-

d)

Mg2+ S2-

39.

Make the magnitude of the charge on each ion (without the sign) become the subscript for the opposite ion.

a)

Switch the subscripts of the ions.

b)

Keep the subscripts as they are.

c)

Double the subscripts of the ions.

d)

Remove the subscripts of the ions.

40.

If possible, reduce the subscripts to give a ratio with the smallest whole numbers.

a)

Yes, it is possible

b)

No, it is not possible

41.

Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the anions.

a)

True

b)

False

42.

What is the formula for the polyatomic ion acetate?

a)

C2H3O2−

b)

CH3COO−

c)

C2H4O2

d)

C2H3O−

43.

What is the formula for the polyatomic ion carbonate?

a)

CO3 2−

b)

CO4 2−

c)

CO3 −

d)

CO2 2−

44.

What is the formula for the polyatomic ion hydrogen carbonate (or bicarbonate)?

a)

HCO3−

b)

H2CO3

c)

CO32−CO3^2−

d)

HCO2−

45.

What is the formula for the polyatomic ion hydroxide?

a)

OH−

b)

OH+

c)

O2H−

d)

HO2−

46.

What is the formula for the polyatomic ion nitrate?

a)

NO3−

b)

NO2−

c)

NO4−

d)

N2O5

47.

What is the formula for the polyatomic ion nitrite?

a)

NO2−

b)

NO3−

c)

NH4+

d)

SO42−SO4^2−

48.

What is the formula for the polyatomic ion chromate?

a)

CrO4 2−

b)

Cr2O7 2−

c)

CrO3 −

d)

CrO2 −

49.

What is the formula for the polyatomic ion dichromate?

a)

Cr2O7 2−

b)

CrO4 2−

c)

Cr2O4 2−

d)

CrO7 2−

50.

What is the formula for the polyatomic ion phosphate?

a)

PO4 3−

b)

PO3 3−

c)

PO4 2−

d)

PO3 2−

51.

What is the formula for the polyatomic ion hydrogen phosphate?

a)

HPO4 2−

b)

H2PO4 −

c)

PO4 3−

d)

H3PO4

52.

What is the formula for the polyatomic ion ammonium?

a)

NH4+

b)

NH3

c)

NH2-

d)

NH4-

53.

What is the formula for the polyatomic ion hypochlorite?

a)

ClO−

b)

ClO2−

c)

ClO3−

d)

ClO4−

54.

What is the formula for the polyatomic ion chlorite?

a)

ClO2−

b)

ClO3−

c)

ClO−

d)

ClO4−

55.

What is the formula for the polyatomic ion chlorate?

a)

ClO3−

b)

ClO2−

c)

ClO4−

d)

ClO−

56.

What is the formula for the polyatomic ion perchlorate?

a)

ClO4−

b)

ClO3−

c)

ClO2−

d)

ClO−

57.

What is the formula for the polyatomic ion permanganate?

a)

MnO4−

b)

MnO3−

c)

MnO2−

d)

MnO−

58.

What is the formula for the polyatomic ion sulfate?

a)

SO4 2−

b)

SO3 2−

c)

SO4 3−

d)

S2O4 2−

59.

What is the formula for the polyatomic ion sulfite?

a)

SO3 2−

b)

SO4 2−

c)

SO2 2−

d)

S2O3 2−

60.

Write a formula for the compound that forms from zinc and nitrate. Follow these steps: 1. Write the symbol for the metal and its charge followed by the symbol of the polyatomic ion and its charge. 2. Use the magnitude of the charge on each ion as the subscript for the other ion. 3. If possible, reduce the subscripts to give a ratio with the smallest whole numbers. 4. Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the anions.

a)

Zn(NO3)2

b)

Zn2(NO3)2

c)

Zn(NO3)

d)

Zn2NO3

61.

The formula for the compound that forms from zinc and nitrate is ____.

a)

Zn(NO3)2

b)

ZnNO3

c)

Zn2(NO3)3

d)

Zn(NO2)2

62.

Write a formula for the compound that forms from Sodium and Sulfite ions. Follow these steps: 1. Write the symbol for the metal and its charge followed by the symbol of the polyatomic ion and its charge. [You need to memorize polyatomic ions and their charges; Table 5.3] 2. Use the magnitude of the charge on each ion as the subscript for the other ion. 3. If possible, reduce the subscripts to give a ratio with the smallest whole numbers. 4. Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the anions.

a)

Na2SO3

b)

NaSO3

c)

Na2(SO3)2

d)

Na3SO3

63.

Write a formula for the compound that forms from aluminum and phosphate.

a)

AlPO4

b)

Al2(PO4)3

c)

Al3(PO4)2

d)

Al(PO4)2

64.

Write the symbol for the metal and its charge followed by the symbol of the polyatomic ion and its charge. [You need to memorize polyatomic ions and their charges; Table 5.3]

a)

Na+ NO3-

b)

K+SO42−K + SO_4^{2-}

c)

Ca2+CO32−Ca^2+ CO3^2-

d)

Mg2+PO43−Mg^2+ PO4^3-

65.

What is the formula for the compound that forms from magnesium and hydroxide?

a)

Mg(OH)2

b)

MgO

c)

MgH2

d)

Mg(OH)

66.

Check to make sure that the sum of the charges of the cations exactly cancels the sum of the charges of the anions. What is the overall charge?

a)

+1

b)

-1

c)

0

d)

+2

67.

What is the order of elements in a chemical formula based on metallic character?

4 lines
68.

In the chemical formula H2O, what does the subscript '2' indicate?

a)

The subscript '2' in the chemical formula H2O indicates that there are two hydrogen atoms in each molecule of water.

b)

The subscript '2' indicates that there are two oxygen atoms in each molecule of water.

c)

The subscript '2' indicates that there are two molecules of water.

d)

The subscript '2' indicates that there are two atoms of hydrogen and oxygen combined in each molecule of water.

69.

What does the subscript '2' in Mg(NO3)2 indicate?

a)

It indicates there are two nitrate ions (NO3-) for each magnesium ion (Mg2+).

b)

It indicates there are two magnesium ions (Mg2+) for each nitrate ion (NO3-).

c)

It indicates the compound is diatomic.

d)

It indicates the presence of two oxygen atoms.

70.

True or False: In chemical formulas, a metal is usually followed by a non-metal.

a)

True

b)

False

71.

What is the basic unit of atomic elements?

a)

Molecules

b)

Single atoms

c)

Compounds

d)

Ions

72.

How many total molecular elements are there to memorize?

a)

5

b)

6

c)

7

d)

8

73.

Ionic compounds are generally composed of _______.

a)

metal + nonmetal

b)

nonmetal + nonmetal

c)

metal + metal

d)

noble gas + metal

74.

Molecular compounds are formed from two or more _______.

a)

nonmetals

b)

metals

c)

metalloids

d)

noble gases

75.

What type of bond is found in molecular compounds?

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

76.

What is the chemical formula for water?

a)

H2O

b)

H2O2

c)

CO2

d)

NaCl

77.

What is the systematic name for H2O?

a)

Water

b)

Hydrogen Dioxide

c)

Dihydrogen Monoxide

d)

Hydroxide

78.

By knowing the rules of nomenclature, you can examine a compound’s formula and determine its name or vice versa.

a)

True

b)

False

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