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Chemistry Semester 1 Review

Total questions: 76

Worksheet time: 58mins

Name
Class
Date
1.
Which is not a pure substance?
a)
Milk
b)
Oxygen
c)
Water
d)
Carbon doxide
2.

Which of the following is a physical change?

a)

Burning wood

b)

Baking a cake

c)

Melting ice

d)

Sulfuric acid reacting with sugar

3.

Which of the follow indicates a chemical change?

a)

Change in shape

b)

Change in volume

c)

Change in temperature

d)

Change in chemical composition

4.

Which of the following is a physical property?

a)

Density

b)

Flammability

c)

Reactivity

d)

Radioactivity

5.

Which of the following is a chemical property

a)

Melting point

b)

Density

c)

Malleability

d)

Flammability

6.

Properties that DO depend on the amount of matter present.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

7.

Properties that depend on the identity of substance.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

8.

Which of the following is an extensive property?

a)

Color

b)

Mass

c)

Odor

d)

Luster

9.

The state of matter with no definite shape but a definite volume is

a)

solid

b)

liquid

c)

gas

d)

all 3

10.

The particles of a solid are typically

a)

compressed

b)

far apart and move about freely

11.

Which of the following can be separated using physical means?

a)

compounds

b)

elements

c)

pure substances

d)

mixtures

12.
It feels smooth.
a)
Qualitative 
b)
Quantitative
13.
The temperature of the room is decreasing by 4 degrees Celsius.
a)
Qualitative
b)
Quantitative
14.
Jack has a rock. The rock has a mass of 14g and a volume of 2cm3. What is the density of the rock?
a)
7 mL
b)
7 g/cm3
c)
28 g/cm3
d)
1/7 g/cm3
15.
What is the volume of Object X?
a)
10.0 cm3
b)
15.0 cm3
c)
20.0 cm3
d)
25.0 cm3
16.

What is the volume of 150 grams of lead if it has a density of 11.3 g/cm3?

a)

13.3 g

b)

13.3 cm3

c)

.075 g

d)

1695 cm3

17.

How close a measurement is to the true value is called..

a)

Accuracy

b)

Precision

c)

Significant

d)

Estimate

18.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
19.

3200 g is equal to

a)

32 kg

b)

0.32 kg

c)

3.2 kg

d)

320 kg

20.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
21.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
22.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
23.

0.0093 in scientific notation is

a)

93 x 10-4

b)

9.3 x 10-3

c)

93 x 104

d)

9.3 x 103

24.
One of Dalton's conclusions concerning his atomic theory was that all the atoms of different elements are _______.
a)
the same
b)
combined
c)
reacted
d)
different
25.

What scientist is best known for his "Plum Pudding" model of the atom used the cathode ray experiment to discover electrons?

a)

J.J. Tomson

b)

Ernest Rutherford

c)

John Dalton

d)

Democritus

26.

Isotopes have the same mass but different numbers of

a)

protons

b)

neutrons

c)

electrons

d)

all of the above

27.

Number of protons + number of neutrons =

a)

average atomic mass

b)

mass number

c)

atomic number

28.

At atom of phosphorus has a mass number of 31 and an atomic number of 15. How many neutrons does the atom have?

a)

15

b)

16

c)

31

d)

46

29.

How do we get mass from moles?

a)

multiply by avogadro's number

b)

multiply by molar mass

c)

divide by avogadro's number

d)

divide by molar mass

30.
What is the total mass in grams of 0.75 mole of SO2?
a)
16 g
b)
24 g
c)
32 g
d)
48 g
31.

Low energy waves have

a)

long wavelengths

b)

short wavelengths

c)

high frequencies

32.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
33.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
34.

Mosely arranged his periodic table in order of increasing

a)

atomic mass

b)

atomic number

c)

number of neutrons

d)

atomic radius

35.

What period and group is Chlorine (Cl)?

a)

Period 3, Group 14

b)

Period 3, Group 17

c)

Period 2, Group 17

d)

Period 2, Group 14

36.

Who organized the first periodic table?

a)

Mendeleev

b)

Moseley

c)

Mozart

d)

Lavosier

37.

Which group of the periodic table is composed of inert (unreactive) gases?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

38.

What is on the left side of the dark line on the periodic table?

a)

Non-Metals

b)

Metals

c)

Metalloids

d)

Anions

39.

Which is a halogen?

a)

Helium

b)

Chlorine

c)

Oxygen

d)

Niobium

40.

How many valance electrons does iodine have?

a)

6

b)

16

c)

7

d)

17

41.

Which atom has the largest atomic radius?

a)

magnesium

b)

chlorine

c)

barium

d)

selenium

42.

The element with the largest electron affinity is:

a)

At

b)

F

c)

Cl

d)

Br

43.

As we go from the left side to the right side on the periodic table, electronegativity:

a)

Increases

b)

Decreases

c)

Remains constant

44.

Elements are arranged on the periodic table according to similarity of properties because of this law

a)

conservation of mass

b)

conservation of energy

c)

atomic law

d)

periodic law

45.

The energy required to remove the most loosely bound electron is the definition of:

a)

Electronegativity

b)

Electron Affinity

c)

Atomic Radius

d)

Ionization Energy

46.

This group on the periodic table represents the most reactive nonmetals on the periodic table

a)

halogens

b)

noble gases

c)

carbon group

d)

oxygen group

47.

The most unreactive group on the periodic table

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

48.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

49.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

50.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

51.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

52.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

53.

Magnesium Hydroxide is an ionic compound made up from Mg2+ and OH- ions. Which is its correct formula?

a)

MgOH

b)

MgOH2

c)

Mg(OH)2

d)

MgO

54.

Calcium Fluoride has a chemical formula of CaF2. What does the chemical formula tell you?

a)

There are 2 Calcium ions for every 1 Fluoride ion in the crystal

b)

There is 1 Calcium ion for every 2 Fluoride ions in the crystal

55.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
56.
Write the formula for barium + nitrogen
a)
Ba2N3
b)
Ba3N2
c)
BaN
d)
BaN3
57.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
58.
Write the correct formula for an ionic compound formed from S2- and Rb1+.
a)
SRb2
b)
SRb
c)
Rb2S
d)
RbS2
59.

Which of the following will form an anion?

a)

metal

b)

nonmetal

60.

Which of the following will form a cation?

a)

metal

b)

nonmetal

61.

Name the following compound: FeCl2

a)

Iron chlorine

b)

Iron chloride

c)

Iron (I) chloride

d)

Iron (II) Chloride

62.

What is the chemical formula for the covalent compound: nitrogen monoxide

a)

NO

b)

NO2

c)

N2O

d)

O

63.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
64.

Which of the following is the best representation of a molecule of fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

65.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
66.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
67.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

68.

Silicon dioxide is the compound in sand. What is its formula?

a)

SO2

b)

NaO2

c)

SiO2

d)

SiO

69.

The correct name for CH4 is...

a)

Carbon Hydrogen

b)

Carbon Tetrahydride

c)

Monocarbon hydride

d)

Carbon Hydride

70.

Which of the following names matches the chemical formula N2O3?

a)

Dinitrogen triople oxide

b)

Nitrogen oxide

c)

Dinitrogen trioxide

d)

Trioxide nitrogen

71.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
72.

When two atoms are bonded covalently and they share electrons equally they form

a)

an ionic bond

b)

a polar covalent bond

c)

a non-polar covalent bond

73.

What shape will the molecule PCl3 form?

a)

trigonal planar

b)

trigonal pyramidal

c)

tetrahedral

d)

bent

74.

What shape will the molecule HF form?

a)

linear

b)

bent

c)

tetrahedral

d)

trigonal planar

75.

What are the most common types of radioactive decay

a)

alpha

b)

beta

c)

gamma

d)

all of the above

76.

Which of the following best describes the difference between fusion and fission?

a)

Fission is combining nuclei and fusion is splitting nuclei

b)

Fission is splitting nuclei and fusion is combining nuclei

c)

Fusion and fission are identical

d)

Fusion and fission are not types of nuclear radiation

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