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Chemistry Midterm Review

Total questions: 80

Worksheet time: 1hrs 19mins

Name
Class
Date
1.

As the elements in Group 2 in the periodic table are considered in order of increasing atomic number, there is a general increase in

a)

stability

b)

atomic radius

c)

electronegativity

d)

first ionization energy

2.

How many electron pairs are shared between the atoms in an N2 molecule?

a)

1

b)

2

c)

3

d)

4

3.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

4.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

5.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

6.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

7.

What quantity is the same among atoms of the same element?

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of nucleons

8.

An atom that has 8 protons and 10 neutrons is an isotope of the element

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

9.

Which elements have the most similar chemical properties?

a)

Ge, As, and Sb

b)

Mn, Fe, and Co

c)

S, Se, and Te

d)

P, S, and Cl

10.

Which atom has the lowest electronegativity?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

11.

Which temperature is equal to 170 C?

a)

103 K

b)

443 K

c)

-103 K

d)

498 K

12.

What is the overall charge of an ion that has 9 protons, 11 neutrons, and 10 electrons?

a)

+1

b)

-1

c)

+2

d)

-2

13.

What are 3 examples of metals:

a)

Lithium

Sodium

Calcium

b)

Nitrogen

Oxygen

Fluorine

c)

Helium

Neon

Argon

14.

What is the correct Lewis dot structure for Selenium:

a)
b)
c)
15.

Why is the image the correct Lewis dot for Selenium?

a)

It is in group 1, with 1 valence electron

b)

It is group 2, with 2 valence electrons

c)

It is in group 16, with 6 valence electrons

16.

Which element is this Bohr diagram from?

a)

Selenium, because it has 34 electrons

b)

Sulfur, because it has 16 electrons

c)

Sodium, because it has 11 electrons

17.

Which elements are examples of Alkali Earth Metals?

a)

Lithium, Sodium

b)

Beryllium, Magnesium

c)

Boron Aluminum

18.

How do you find the number of valence electrons?

a)

atomic number

b)

group number

c)

period number

19.

A substance that is tightly packed together is most likely in what state of matter?

a)

solid

b)

liquid

c)

gas

20.

Approved eye protection devices (such as goggles) are worn in the laboratory

a)

to avoid eye strain.

b)

to improve your vision.

c)

only if you don’t have corrective glasses.

d)

any time chemicals, heat or glassware are used.

21.

If you do not understand a direction or part of a lab procedure, you should

a)

figure it out as you do the lab.

b)

try several methods until something works.

c)

ask the instructor before proceeding.

d)

skip it and go on to the next part.

22.

Work areas should be kept clean and tidy.

a)

True

b)

False

23.

Read all procedures thoroughly before entering the laboratory.

a)

True

b)

False

24.

Which of the following is not part of the atomic theory?

a)

All matter is composed of tiny, invisible, indivisible particles called atoms

b)

Atoms of different elements are different.

c)

Atoms have a neutral charge

d)

Atoms of the same element are the same.

e)

Atoms cannot be created or destroyed, just rearranged.

25.

What subatomic particle has a positive charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Neutron- nucleus

d)

Neutron- outside nucleus

26.

What subatomic particle has a negative charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Electron- nucleus

d)

Electron- outside nucleus

27.

What subatomic particle has a neutral charge in the atom? Where is it located?

a)

Proton- nucleus

b)

Proton- outside nucleus

c)

Neutron- nucleus

d)

Neutron- outside nucleus

28.

What is the atomic number?

a)

Number of protons

b)

Number of neutrons

c)

Number of protons + neutrons

29.

What is the mass number?

a)

Number of protons

b)

Number of neutrons

c)

Number of protons + neutrons

30.

What is an isotope?

a)

Same element with different number of protons

b)

Same element with different number of neutrons

c)

Same element with different number of electrons

d)

Different elements

31.

What does the “Na” represent?

a)

Atomic number

b)

Mass number

c)

Element symbol

d)

Element name

32.

What does the “Sodium” represent?

a)

Atomic number

b)

Mass number

c)

Element symbol

d)

Element name

33.

What does the “11” represent?

a)

Atomic number

b)

Mass number

c)

Element symbol

d)

Element name

34.

Who discovered the proton?

a)

Chadwick

b)

Mendeleev

c)

Rutherford

d)

Dalton

35.

Who discovered the neutron?

a)

Chadwick

b)

Thompson

c)

Rutherford

d)

Dalton

36.

Who first coined the word, "Atomos"?

a)

Democritus

b)

Dalton

c)

Mendeleev

d)

Thompson

37.

How many electrons does the element nitrogen have?

a)

14

b)

7

c)

14

d)

21

38.

How many protons does gold have?

a)

79

b)

196

c)

39.5

d)

30

39.

True or False: The two rows at the bottom of the periodic table are apart of groups 6 and 7?

a)

True

b)

False

40.

How many groups are on the periodic table?

a)

16

b)

7

c)

18

d)

6

41.

How many periods are on the periodic table?

a)

7

b)

18

c)

16

d)

6

42.

Which element is in Period 2 and Group 13?

a)

Boron

b)

Nitrogen

c)

Carbon

d)

Oxygen

43.

Which element is in period 3, group 1?

a)

Magnesium

b)

Lithium

c)

Carbon

d)

Sodium

44.

Which of the following elements is a nonmetal?

a)

Helium

b)

Boron

c)

Silicon

d)

Gold

45.

Which of the following elements is considered a metal?

a)

Iron

b)

Gold

c)

Silver

d)

All of the above

46.

Which subatomic particle carries a positive charge?

a)

Proton

b)

Electron

c)

Neutron

d)

None of the above

47.

Which of the following carries a negative charge?

a)

Proton

b)

Neutron

c)

Electron

48.

Which group contains the Noble Gas Family?

a)

7

b)

17

c)

18

d)

3

49.

Which group contains the alkali metal family?

a)

Group 2

b)

Group 1

c)

Group 3

d)

Group 18

50.

Which group contains Helium?

a)

Group 1

b)

Group 2

c)

Group 3

d)

Group 18

51.

How many valence electrons does Magnesium have?

a)

1

b)

2

c)

3

d)

4

52.

How many valence electrons are in group 13?

a)

3

b)

2

c)

13

d)

1

53.

Which group contains the element Silicon?

a)

2

b)

1

c)

14

d)

13

54.

True or False: Mendeleev knew the properties of the elements that weren't discovered yet.

a)

True

b)

False

55.

True or False: Elements that are known as metalloids share the same characteristics as both metals and nonmetals.

a)

True

b)

False

56.

How many elements are on the Periodic Table?

a)

100

b)

117

c)

119

d)

118

57.

True or False: The atomic number is the same as the number of neutrons.

a)

True

b)

False

58.

How many protons are found in an oxygen atom (#8)?

a)

2

b)

6

c)

4

d)

8

59.

The smallest particle of an element that retains the properties of that element is a(n) ____.

a)

electron

b)

proton

c)

atom

d)

neutron

60.

In Bohr's model of the atom, where are the electrons and protons located?

a)

The electrons occupy fixed positions around the protons, which are at the center of the atom.

b)

The electrons and protons move throughout the atom.

c)

The electrons and protons are located throughout the atom, but they are not free to move.

d)

The electrons move around the protons, which are at the center of the atom.

61.

Why are atoms electrically neutral?

a)

They contain equal numbers of protons and neutrons.

b)

They contain more neutrons than protons.

c)

They contain more electrons than protons.

d)

They contain equal numbers of protons and electrons.

62.

Most metals are NOT:

a)

ductile

b)

malleable

c)

good conductors

d)

liquid at room temperature

63.

Which state of matter is characterized by having a definite shape and a definite volume?

a)

solid

b)

liquid

c)

gas

d)

plasma

64.

Which general electron configuration is responsible for the family properties of noble gases?

a)

ns2

b)

ns2np6

c)

ns2np5

d)

ns2np4

e)

ns1

65.

Which of the following items is considered a heterogeneous mixture?

a)

kool-aid

b)

coffee

c)

salad

d)

vinegar

66.

Isotopes of the same element have different ____.

a)

atomic numbers

b)

chemical behavior

c)

mass numbers

d)

positions on the periodic table

67.

What is the electron configuration of potassium?

a)

1s22s22p63s23p64s2

b)

1s22s22p63s23p64s1

c)

1s22s23s23p63d1

d)

1s22s22p63s23p6

68.

What are the substances that are found at the end of a reaction called?

a)

acids

b)

chemicals

c)

reactants

d)

products

69.

What refers to any electrically neutral group of atoms that are bound together?

a)

Chemical bond

b)

Molecular compound

c)

Molecule

d)

Compound

70.

What refers to a chemical compound (2 or more atoms) whose simplest units are molecules?

a)

Chemical bond

b)

Molecular compound

c)

Molecule

d)

Compound

71.

Describe a covalent bond.

a)

A bond where electrons are gained or lost

b)

A bond between two metals

c)

A bond where electrons are shared

72.

Describe an ionic bond.

a)

A bond where electrons are gained or lost

b)

A bond between two metals

c)

A bond where electrons are shared

73.

What is the octet rule?

a)

When an atom has 8 electrons in the outer valence shell

b)

When you have 8 arms

c)

When an atom has a total of 8 electrons

d)

When an atom has more than 8 total electrons

74.

What are models that show all bonding and non-bonding (lone pair) electrons of each atom within a molecule or atom?

a)

Bohr model

b)

Lewis dot

c)

Chemical formula

75.

What represents shared electrons between valence shells of atoms?

a)

Paired dots

b)

Paired stars

c)

Single dots

d)

Single stars

76.

If an element is in group 13, how many valence electrons does it have?

a)

2

b)

3

c)

6

d)

7

77.

If an element is in group 16, how many valence electrons does it have?

a)

2

b)

3

c)

6

d)

7

78.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

79.
Why does K become positive when it bonds to Cl to form KCl?
a)
Because it loses an electron to have a full valence shell 
b)
Because it gains an electron to have 2 valence electrons
c)
Because it loses an electron to become negatively charged
d)
Because Cl gives away its 7 electrons to Na to form an equal charge 
80.
What is a cation? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge

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