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Worksheets

(CHM) Mid Year 21-22

Total questions: 69

Worksheet time: 1hrs 13mins

Name
Class
Date
1.

Convert 360 s to ms

a)

3,600 ms

b)

36,000 ms

c)

0.36000 ms

d)

360,000 ms

2.

Convert 4800 mg to kg

a)

48 kg

b)

0.0048 kg

c)

0.048 kg

d)

4.8 kg

3.

The metric system is based or scaled on units of:

a)

ten

b)

100

c)

1000

d)

inches

4.
Given that 1 yard is approximately 0.914 meter, 50 yards would be equivalent to approximately how many meters?
a)
45.7 meters
b)
49.09 meters
c)
50.91 meters
d)
54.7 meters
5.
45 cm = ___ mm
a)
450 mm
b)
4,500 mm
c)
45 mm
d)
4.5 mm
6.

Does this image show results that are accurate and/or precise?

a)

Accurate, but not precise

b)

Precise, but not accurate

c)

Both precise and accurate

d)

Neither precise nor accurate

7.
The attendance for the basketball game was estimated to be 15,000 people but 12,500 people attended. What was the percent error?
a)
16.67%
b)
20%
c)
2500%
d)
80%
8.
The deer population is estimated to be 17,600 in northern Illinois, but an actual count was 21,300. What is the percent error?
a)
21%
b)
17.37%
c)
17.4%
d)
21.02%
9.

Which of the following has 5 significant figures?

a)

0.000 5 cm

b)

0.000 05 cm

c)

10 005 cm

d)

1 005 550 cm

10.
Calculate 1.23 m x 0.89 m and give your answer with the correct number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.095 m2
11.
Try to change the number back to standard form:  6.79  x  104
a)
679,000
b)
6,790
c)
67,900
d)
6,790,000
12.
Approximately 5 miles=8 kilometers. About how many miles are 1019 kilometers?
a)
1,250
b)
1,000
c)
625
d)
500
13.

Properties that depend on the identity of substance.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

14.

Properties that DO depend on the amount of matter present.

a)

Mass

b)

Hardness

c)

Extensive

d)

Intensive

15.
Example for chemical property
a)
color
b)
hardness
c)
toxicity
d)
solubility
16.

An _______________ is made up of one or more of the same kind of atom chemically combined.

a)

atom

b)

element

c)

molecule

d)

compound

17.

A ______________ mixture is one that does not have a uniform composition.

a)

heterogeneous

b)

homogenous

c)

pure substance

18.

A _________________ mixture is one where the substances are evenly spread throughout.

a)

heterogeneous

b)

homogeneous

c)

pure substance

19.
This diagram represents a _____.
a)
pure substance that is a compound
b)
mixture of elements
c)
pure substance that is an element
d)
mixture of compounds
20.

What technique is being carried out in the picture?

a)

crystallization

b)

sublimation

c)

chromatography

d)

sedimentation

21.

J.J. Thomson discovered the electron using

a)

gold foil and alpha particles.

b)

oil drops.

c)

a cathode ray tube.

d)

emission spectra of a hydrogen atom.

22.

Which of these experiments supported the idea of electrons?

a)
b)
c)
d)
23.

Which of these experiments supported the idea of a small nucleus?

a)
b)
c)
d)
24.

Different isotopes have...

a)

different mass numbers

b)

different protons

c)

different electrons

d)

different atomic numbers

25.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
26.

This image is an illustration of

a)

photoelectric effect

b)

Dalton's atomic theory

c)

Bohr model

d)

Quantum mechanical model

27.

The figure shows _____________

a)

atomic emission spectrum

b)

atomic absorption spectrum

c)

atomic solution spectrum

d)

photoelectric effect

28.

Calculate the energy of a gamma ray photon whose frequency is 5.02 x 1020/s?

E=hvE=hv  h = 6.63 x 10-34 J*s

a)

4.73 x 1072 J

b)

2.07 x 10 6 J

c)

3.33 x 10-13 J

d)

1.21 x 10 35 J

29.

What is the energy of light whose wavelength is 4.06 x 10-11 m?

c=λvc=\lambda v  c = 3.00 x 108 m/s

E=hvE=hv  h = 6.63 x 10-34 J*s

a)

2.69 x 10-44 J

b)

4.90 x 10-15 J

c)

3.06 x 10 4 J

d)

5.04 x 10-17 J

30.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

31.
The position & momentum of the electron cannot be known at the same time. 
a)
Planck
b)
Heisenberg
c)
de Broglie
d)
Schrodinger
32.
The second energy level (n=2) contains a total of 5 electrons...how many more electrons can fit in the 2nd energy level?
a)
0
b)
3
c)
5
d)
7
33.

Photoelectric effect provides the evidence for the ______ nature of radiation.

a)

dual

b)

wave

c)

particle

d)

electromagnetic

34.

Light is emitted when electrons

a)

move from one atom to another.

b)

collide with one another, releasing energy.

c)

move from a lower energy level to a higher energy level.

d)

move from a higher energy level to a lower energy level.

35.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
36.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
37.

What is the electron configuration of potassium (K)?

a)

1s22s22p63s1

b)

1s22s22p63s23p64s1

c)

1s22s22p63s23p3

d)

1s22s22p63s23p1

38.

According to the Aufbau principle _____.

a)

an orbital may be occupied by only two electrons

b)

electrons enter orbitals of highest energy first

c)

electrons enter orbitals of lowest energy first

d)

electrons in the same orbital must have opposite spins

39.

Which electron configuration correctly represents the ground state of bromine?

a)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p5

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d9 4p6

d)

1s2 2s2 2p6 3s2 3p6 4s2 4d9 4p6

40.

Identify the correct the electron dot diagram for lithium

a)
b)
c)
d)
41.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
42.

K ionizes to a charge of _________.

a)

+1

b)

+2

c)

-1

d)

-2

43.

Mg ionizes to a charge of ______.

a)

+1

b)

+2

c)

-1

d)

-2

44.

Which types of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

45.

Which types of elements form anions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

46.

Name the following ionic compound: MgSO4

a)

magnesium sulfoxide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium oxide

47.

The formula of calcium phosphate is 

a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
48.
The chemical compound for sodium phosphate would be:
a)
NaPO4
b)
Na2PO4
c)
Na3PO4
d)
Na(PO4)3
49.
NH4 +1  and  C2O4 -2
a)
NH4C2O4
b)
(NH4)2C2O4
c)
NH4(C2O4)2
d)
correct answer is not given
50.
The correct chemical formula for magnesium phosphide is
a)
MgP
b)
Mg₂P₃
c)
Mg₃P₂
d)
Mg₃(PO₄)₂
51.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
52.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
53.

What is the correct formula for Ammonium phosphate?

a)

NH4PO4

b)

NH43PO4

c)

(NH4)3PO4

d)

NH4(PO4)3

54.

What is the correct formula for the polyatomic ion called sulfate?

a)

SO32–

b)

HSO4–

c)

SO42–

d)

CH3COO–

55.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
56.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
57.
What is the formula for iron(II) carbonate?
a)
Fe2CO3
b)
FeCO3
c)

Fe2CO2

d)

FeCO4

58.
Name the Compound:
SnO2
a)
tin(II) oxide
b)
tin(IV)oxide
c)
tin(II)oxegen 
d)
tin oxide
59.

PbS2

a)

lead sulfide

b)

lead sulfur

c)

lead(II) sulfide

d)

lead(IV) sulfide

60.

Name Fe(NO3)3

a)

Iron(III) Nitrate

b)

Iron(III) Nitrite

c)

Iron Nitrite(III)

d)

Iron Nitrate

e)

Iron Oxynitride

61.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
62.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
63.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

64.

Why are metals malleable? (They can bend without breaking.)

a)

Metals are very smooth.

b)

Metals have a sea of electrons.

c)

The sea of electrons form a strong metallic bond.

d)

Even though the metal ions repel each other, the electron sea holds all the atoms in place.

65.

Why are metals good conductors of electricity?

a)

The electric current can easily travel along the surface of the metal because it is smooth.

b)

A negative charge can easily push the sea of electrons in one direction, making a current.

c)

Metals attract electricity.

d)

Metals are malleable.

66.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
67.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
68.

What is the correct Lewis structure for H2CO3?

a)
b)
c)
d)
69.

Which is a correct Lewis structure for HNO3?

a)
b)
c)
d)

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