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Chemistry Semester 1 Exam Review

Total questions: 53

Worksheet time: 47mins

Name
Class
Date
1.

The closeness of a measurement to its true value is a measure of its:

a)

Usefulness

b)

Precision

c)

Accuracy

d)

Reproducibility

2.

The metric unit of volume is:

a)

L

b)

mg

c)

km

d)

K

3.

The number of neutrons in the nucleus of an atom can be calculated by:

a)

electrons + protons

b)

electrons - protons

c)

mass number - protons

d)

mass number + protons

4.

Atomic masses are measured in:

a)

nanograms

b)

grams

c)

angstroms

d)

amu

5.

Which of the following is a metalloid?

a)

As

b)

O

c)

Br

d)

Kr

6.

What is the term for quanta of light?

a)

Charms

b)

Excitons

c)

Muons

d)

Photon

7.

The distance between two consecutive peaks or troughs in a wave is:

a)

Frequency

b)

Wavelength

c)

Quantization

d)

Photon

8.

Who developed a quantum model for the hydrogen atom?

a)

Rutherford

b)

Albert Einstein

c)

Niels Bohr

d)

Max Planck

9.

Which scientists contributed to the development of quantum mechanics?

a)

Werner Heisenberg

b)

Louis de Broglie

c)

Max Planck

d)

Erwin Schrodinger

10.

In a given atom, no two electrons can have the same set of four quantum numbers. This is known as:

a)

Probability distribution

b)

Radial probability distribution

c)

Quantum mechanical model

d)

Pauli exclusion principle

11.

Chemistry is the study of

a)

chemicals and chemical reactions

b)

carrying out experiments

c)

smelly experiments

d)

the universe

12.

An atom is:

a)

any small simple particle

b)

a small unit particle of an element

c)

a small unit particle of a compound

d)

a molecule

13.

What is a compound?

a)

A simple chemical

b)

A simple chemical made of one type of atom

c)

A simple chemical made up of two different types of atoms

d)

A simple chemical made up of different types of atoms

14.

What is the basic unit of a chemical element?

a)

Atom

b)

Proton

c)

Element

d)

Ductile

15.

The positively charged central core of an atom, consisting of protons and neutrons, contains nearly all its mass. What is it called?

a)

Nucleus

b)

Non-metal

c)

Proton

d)

Corrosion

16.

A stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity in solids.

a)

Electron

b)

Proton

c)

Neutron

d)

Nucleus

17.

The number of protons in the nucleus of an atom determines the chemical properties of an element and its place in the periodic table.

a)

Atomic number

b)

Mass number

c)

Group/Family

d)

Reactivity

18.

An abbreviation or short representation of a chemical element; the symbols in the periodic table.

a)

Chemical Symbol

b)

Periodic Table

c)

Malleable

d)

Luster

19.
The name given to a horizontal row of the periodic table. The periodic table has seven. 
a)
Period
b)
Group/Family
c)
Magnetism
d)
Molecule
20.

A group of atoms bonded together represents the smallest fundamental unit of a chemical compound that can take part in a chemical reaction.

a)

Molecule

b)

Atom

c)

Nucleus

d)

Metalloid

21.
An element (e.g., germanium or silicon) whose properties are intermediate between those of metals and solid nonmetals. 
a)
Metal
b)
Metalloid
c)
Non-metal
d)
Period
22.
The ability of a substance, usually a metal, to be deformed or molded into a different shape.
a)
Malleable
b)
Metalloid
c)
Luster
d)
Ductile
23.

A measure of volume is:

a)

Molarity

b)

Grams

c)

Moles

d)

Liters

24.

What is a measure of mass?

a)

Molarity

b)

Grams

c)

Moles

d)

Volume

25.

A charged atom is known as:

a)

Ion

b)

Element

c)

Mutant

d)

Plant

26.

A positively charged atom is known as:

a)

Ion

b)

Cation

c)

Anion

d)

Polyatomic ion

27.

Which rule states that atoms gain, lose, or share electrons to acquire eight valence electrons?

a)

Octet Rule

b)

Quartet Rule

c)

Octo-electron Rule

28.

Which atomic structure depicts electrons in their energy levels (shells)?

a)

Plum Pudding Model

b)

Lewis Dot Structure

c)

Bohr Model

29.

Which diagram shows the bonding between atoms of a molecule and pairs of electrons?

a)

Skeletal Structure

b)

Periodic Table

c)

Lewis Dot Structure

30.

Which form of an element contains the same number of protons, but a different number of neutrons?

a)

Isotope

b)

Iostype

c)

Atom

31.

What type of electron is in the outermost shell of an atom?

a)

Nucleus

b)

Balanced

c)

Valence

32.

The number of protons and neutrons in an atom are equivalent to...

a)

Atomic Number

b)

Atomic Mass

c)

Atomic Symbol

33.

The number of protons in an atom is equivalent to its ____________.

a)

Atomic Mass

b)

Atomic Symbol

c)

Atomic Number

34.

Which form of an element contains the same number of protons, but a different number of neutrons?

a)

Isotope

b)

Iostype

c)

Atom

35.

A stable subatomic particle occurring in all atomic nuclei, with a positive electric charge equal in magnitude to that of an electron, but of opposite sign.

a)

Neutron

b)

Proton

c)

Period

d)

Luster

36.

A stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity in solids.

a)

Electron

b)

Proton

c)

Neutron

d)

Nucleus

37.

A subatomic particle of about the same mass as a proton but without an electric charge, present in all atomic nuclei except those of ordinary hydrogen.

a)

Neutron

b)

Nucleus

c)

Proton

d)

Atom

38.

The number of protons in the nucleus of an atom determines the chemical properties of an element and its place in the periodic table.

a)

Atomic number

b)

Mass number

c)

Group/Family

d)

Reactivity

39.
The name given to a horizontal row of the periodic table. The periodic table has seven. 
a)
Period
b)
Group/Family
c)
Magnetism
d)
Molecule
40.
A table of the chemical elements arranged in order of atomic number, usually in rows, so that elements with similar atomic structure (and hence similar chemical properties) appear in vertical columns.
a)
Periodic Table
b)
Chemical Symbol
c)
Period
d)
Conductivity
41.

Which elements generally form an ionic bond?

a)

Metal and nonmetal

b)

Two nonmetals

c)

Metal

d)

None of the above

42.

Which elements generally form a covalent bond?

a)

Metal and nonmetal

b)

Two nonmetals

c)

Metal

d)

None of the above

43.

In chemical compounds, covalent bonds form when:

a)

The electronegativity difference between two atoms is very large.

b)

Electrons are completely transferred between two metals.

c)

Pairs of electrons are shared between two nonmetal atoms.

d)

Two nonmetal atoms are attracted to each other by opposite charges.

44.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
45.

What type of bond is formed by S and Br, using electronegativities?

a)

Ionic

b)

Polar Covalent

c)

Non-polar Covalent

46.

Using electronegativities, determine the type of bond formed by Co and F.

a)

ionic

b)

polar covalent

c)

non-polar covalent

47.

How many electrons does Si contain?

a)

14

b)

28

c)

2

d)

4

48.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
49.

What happens when an atom loses an electron?

a)

It becomes negatively charged

b)

It remains neutral because the proton also leaves

c)

It becomes positively charged

d)

It stays the same

50.

The number of _____ is most important in determining how an atom will bond.

a)

Neutrons

b)

Protons

c)

Valence Electrons

d)

Electrons in the innermost shell

51.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
52.
High Melting & Boiling Points
a)
Ionic
b)
Covalent
53.
Relatively soft
a)
Ionic
b)
Covalent

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