Free Printable Week 6 Exam 1 practice

1.

Is boiling point a physical or chemical property?

a)

Physical property

b)

Chemical property

c)

Biological property

d)

Mechanical property

2.

Classify seawater.

a)

Homogeneous mixture

b)

Element

c)

Compound

d)

Heterogeneous mixture

3.

Write the isotope notation for carbon with 6 protons and 8 neutrons.

a)

14/6 C or ¹⁴C

b)

12/6 C or ¹²C

c)

13/6 C or ¹³C

d)

15/6 C or ¹⁵C

4.

Which has more neutrons: ¹⁴N or ¹⁵N?

a)

¹⁵N

b)

¹⁴N

c)

Both have the same number of neutrons

d)

Neither has neutrons

5.

Which has a lower ionization energy: Mg or Al?

(a)

6.

Calculate molar mass of Al₂(SO₄)₃.

a)

342 g/mol

b)

294 g/mol

c)

318 g/mol

d)

278 g/mol

7.

Write electron configuration of O.

a)

1s² 2s² 2p⁴

b)

1s² 2s² 2p⁶

c)

1s² 2s² 2p²

d)

1s² 2s¹ 2p⁵

8.

Which group tends to form -2 ions?

a)

Group 16 (chalcogens)

b)

Group 1 (alkali metals)

c)

Group 17 (halogens)

d)

Group 2 (alkaline earth metals)

9.

Which element has largest radius: K or Ca?

a)

K

b)

Ca

c)

Na

d)

Mg

10.

Which element has smaller ionization energy: Na or Mg?

a)

Na

b)

Mg

c)

K

d)

Ca

11.

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

12.

How many neutrons are present in the isotope $^{16}_{8}\text{O}$ ?

a)

8

b)

10

c)

16

13.

An element has a mass number of 20 and atomic number of 10. Which is correct?

a)

Neon-20

b)

Calcium-10

c)

Neon-10

d)

Calcium-20

14.

This is an example of a

a)

physical change

b)

chemical change

15.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

16.

Which element is pictured?

a)

neon

b)

fluorine

c)

magnesium

d)

argon

17.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

18.

Based on the data, which number shows the correct location of the element with 2 valence electrons and 3 energy levels.

a)

1

b)

2

c)

3

d)

4

19.

What is the mass in grams of 5.50 × 10¹² atoms of sulfur?

Avogadro's Number = $6.02\times10^{23}\ units\ per\ mole$

molar mass of S = 32.07 g/mol

a)

$2.93\times10^{-10}g$

b)

$5.50\times10^{-10}g$

c)

5.50 g

d)

2.93 g

e)

$3.92\times10^{-12}g$

20.

Which one of the following elements has the smallest atomic radius?

Na, Al, Cl, Mg, P

a)

Na

b)

Cl

c)

Mg

d)

P

e)

Al

21.

Which of the following elements is the most metallic?

Be, K, C, Si, Cs

a)

Cs

b)

K

c)

Be

d)

Si

e)

C

22.

The ground-state electron configuration for manganese (Mn) is ________.

a)

[Ne]4s²3d⁵

b)

[Ar]4s²3d⁵

c)

[Ar]3s²3d⁵

d)

[Ar]4s¹4d⁶

e)

[Ar]4s¹3d⁶

23.

What is the empirical formula of a compound that contains 85.7% carbon and 14.3% hydrogen by mass?

a)

CH₃

b)

C₂H₃

c)

CH

d)

C₃H₆

e)

CH₂

24.

What is the percent composition by mass of hydrogen in methane (CH₄)?

(Atomic weight of C=12, H=1 g/mol)

a)

12.50%

b)

50.00%

c)

20.00%

d)

25.00%

e)

33.33%

25.

What is the order of ionic radius for the following ions?

Na⁺, Mg²⁺, Cl^-, Ca²⁺

a)

Cl^-< Mg²⁺< Na⁺< Ca²⁺

b)

Ca²⁺ < Na⁺< Cl^-< Mg²⁺

c)

Mg²⁺< Na⁺< Ca²⁺ < Cl^-

d)

Na⁺< Cl^-<Mg²⁺< Ca²⁺

26.

Elements in group ________ have a np⁶ electron configuration in the outer shell.

a)

IA

b)

IIIA

c)

VIA

d)

VIIIA

27.

The wavelength of a photon that has an energy of 6.33 × 10^-18 J is ________ m.

$E\ =\frac{h.c}{\lambda}$ $h\ =6.626\times10^{-34}\ J.s\ \ \ \ \ \ \ C\ =3.00\times10^8\ ms^{-1}$

a)

3.10

b)

3.10 × 10^-8

c)

4.21 × 10^-24

d)

3.21 × 10^-12

28.

Which of the following transitions in the Bohr hydrogen atom results in the absorption of the lowest-energy photon?

a)

n = 1 $\rightarrow$ n = 6

b)

n = 6 $\rightarrow$ n = 1

c)

n = 3 $\rightarrow$ n =1

d)

n = 1 $\rightarrow$ n = 3

29.

Benjamin is conducting a chemistry experiment to create a salt by combining the ions Na⁺ and SO₄^2-. He needs to write the correct formula for the salt they form. What is the formula?

a)

Na₃(SO₄)₂

b)

Na₃SO₄

c)

Na₂SO₄

d)

NaSO₄

30.

How many Significant Figures does the number 6.0200 have?

a)

1

b)

2

c)

4

d)

5

e)

3

31.

Oxygen is a __ and Gold is a __.

a)

nonmetal, metal

b)

metal, nonmetal

c)

metal, metal

d)

metalloid, nonmetal

32.

Which one of the following is an extensive property?

a)

temperature

b)

mass

c)

boiling point

d)

melting point

33.

During a science experiment, Maya, Mia, and Isla were given different substances. Maya had liquid mercury, Mia had hydrogen gas, and Isla had a salt solution. Which one of these is an impure substance?

a)

liquid mercury (Maya's substance)

b)

hydrogen gas (Mia's substance)

c)

salt solution (Isla's substance)

d)

elemental gold

34.

Round the number 4.0294894 to the nearest .01

a)

4.02

b)

4.01

c)

4.03

d)

4.029

35.

How many significant figures are in the following number?

1.0200\times10^5

a)

2

b)

3

c)

4

d)

5

36.

Solve. Round using SigFig math rules.
98.7°C - 97.25°C

a)

1°C

b)

1.4°C

c)

1.45°C

d)

1.450°C

37.

Solve. Round using SigFig math rules.
12.5-mL + 20.05-mL + 2.69-mL

a)

35-mL

b)

35.2-mL

c)

35.24-mL

d)

35.240-mL

38.

Solve. Round using SigFig math rules.
0.00040-m × 0.0021-m

a)

0.00000084-m²

b)

0.0000084-m²

c)

8 x 10^-7-m²

d)

8.45 x 10^-7-m²

39.

How many gallons are in a pool that holds 758,000 Liters?
(1 gallon = 3.79 Liters)

a)

200

b)

20,000

c)

200,000

d)

2,000,000

40.

Gas costs $3.05 a gallon, and your car travels at 27 miles for each gallon of gas. How far can you travel in your car with $95 in your pocket?

a)

11 miles

b)

840 miles

c)

7800 miles

d)

870 miles

41.

Elijah earn $200 for 8 hours of work. What is the unit rate (in dollars per hour)?

a)

$50 per hour

b)

$12 per hour

c)

$192 per hour

d)

$25 per hour

42.

Complete the statement:

5.0 cm/min = ______ m/day

(100 cm = 1 m)

a)

72

b)

840

c)

7.2

d)

5,040,000

43.

Jackrabbits are capable of reaching speeds up to 40 miles per hour. How fast is this in feet per second? (Round to the nearest whole number.)

5,280 feet = 1 mile

a)

95 feet per second

b)

59 feet per second

c)

.45 feet per second

d)

40 feet per second

44.

Dry ice has a temperature of -78 ^oC, what is this temperature in Kelvin?

a)

195 K

b)

-351 K

c)

159 K

d)

-213 K

45.

What are the units used to describe formula mass or molar mass?

a)

grams

b)

moles

c)

M

d)

grams/mole

46.

Calculate the volume of metal with a mass of 56.7 grams and a density of 4.67 grams per milliliter.

a)

12.1413276231 mL

b)

12.1 mL

c)

12.1

d)

$264.789\ \frac{g^2}{mL}$

47.

Round off 509.96 to 4 significant figures.

a)

509.9

b)

509.0

c)

510.0

d)

510

48.

The prefix with the scientific notation factor of 10^-6 is:

(a)

49.

The prefix with the scientific notation factor of 10^-3 is:

(a)

50.

A bar of copper has a mass of 216g and a volume of 24 cm³. What is the density of copper?

a)

9 g/cm³

b)

5184 g/cm³

c)

.11 g/cm³

d)

322 mL

51.

If you have a density of 3 g/cm $^3$ and a volume of 4 cm $^3$ , what is the mass?

a)

7 g

b)

12 g

c)

1 g

d)

0.75 g

52.

100 Celsius is ? Kelvin (K = Celsius + 273)

a)

173 K

b)

373K

c)

273 K

d)

0 K

53.

Convert 30°C to Fahrenheit (1.8 x ⁰C) + 32

a)

860°F

b)

86°F

c)

63.8°F

d)

56°F

54.

What is the mass of 0.89 moles of calcium chloride (CaCl₂)?

a)

0.89 g

b)

99 g

c)

99 amu

d)

0.89 amu

55.

How many moles of barium nitrate, Ba(NO₃)₂, contain 6.8 x 10²⁴formula units?

a)

6.02 x 10²³ formula units

b)

11 moles

c)

11 formula units

d)

11 g

56.

How many moles is 397 g of calcium chloride (CaCl₂)?

a)

111 moles

b)

3.58 moles

c)

0.280 moles

d)

44100 moles

57.

What is the empirical formula given the data below?

0.050 mol C

0.150 mol H

0.100 mol O

a)

CHO

b)

CH₂O

c)

CH₃O

d)

CH₃O₂

58.

Identify the number of Chlorine atoms in 65.8 g CaCl_2.

a)

7.14 x 10²³ atoms

b)

8.71 x 10²³ atoms

c)

1.22 x 10²³ atoms

d)

3.57 x 10²³ atoms

59.

How many neutrons does the isotope of lithium have?

a)

8

b)

3

c)

4

d)

5

60.

In a correctly written symbol what would be located in the "A" position?

a)

number of neutrons

b)

atomic number

c)

number of electrons

d)

mass number

61.

Ions are:

a)

atoms with a positive or negative charge

b)

atoms with no charge

c)

atoms with ONLY a positive charge

d)

atoms with ONLY a negative charge

62.

How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?

a)

34

b)

36

c)

2

d)

40

63.

An element's valence electrons are...?

a)

the electrons in all of the shells

b)

the electrons in the highest level / outermost shell

c)

the electrons in the lowest level / innermost shell

d)

none of the above

64.

Potassium has 3 main isotopes. If potassium 39 has an abundance of 93.258%, potassium 40 has an abundance of 0.012% and potassium 41 has an abundance of 6.730%, what is the weighted atomic mass?

a)

39.2

b)

39.0

c)

39.1

d)

39.3

65.

What sublevel holds the most electrons?

a)

s

b)

p

c)

d

d)

f

66.

The first two columns of the periodic table always fill up the _____ sublevels.

a)

s

b)

f

c)

p

d)

d

67.

Find the percent composition of hydrogen in (NH₄)₂S.

a)

11.8%

b)

41.1%

c)

47.1%

68.

How many water molecules are in 5.2 moles of water?

a)

6.02 x 10²³

b)

5.2

c)

3.1304 x 10²⁴

d)

8.638 x 10^-24

69.

What is the mass in grams of 5.90 mol C₈H_18?

a)

.0512 g

b)

19.4 g

c)

673 g

d)

389 g

70.

Which category of elements are found on the far right column of the periodic table (group 18)?

a)

Metalloids

b)

Noble Gases

c)

Alkali Metals

d)

Transition Metals

71.

What determines an element’s atomic number?

a)

The element's mass

b)

The number of neutrons it has

c)

The size of the element

d)

The number of protons it has

72.

Which of these Elements is the largest in Atomic Radius?

a)

Potassium (K)

b)

Oxygen (O)

c)

Lithium (Li)

d)

Bromine (Br)

73.

Elements that share the same number of valence electrons will also have the same _______ number on the Periodic Table.

a)

Period

b)

Atomic number

c)

Angular Momentum

d)

Group

74.

Which of the following values will Increase as you move from left to right on the Periodic Table?

a)

Ionization Energy

b)

Atomic Radius

c)

Electronegativity

d)

Both Ionization Energy and Electronegativity

75.

Which of the following is most reactive?

a)

Lithium

b)

Potassium

c)

Sodium

d)

Cesium

76.

Which color on the image of the periodic table corresponds with the alkaline earth metals.

a)

yellow

b)

dark yellow

c)

blue/green

d)

teal

77.

Which color on the image of the periodic table corresponds with the metalloids.

a)

bright yellow

b)

gold

c)

teal

d)

light blue

78.

Which color on the image of the periodic table corresponds with the transition metals.

a)

red

b)

black

c)

blue

d)

orange

79.

Which color on the image of the periodic table corresponds with the halogens.

a)

red

b)

black

c)

blue

d)

orange

80.

What is ionization energy?

a)

The energy required to remove an electron from a neutral atom of an element.

b)

The energy change that occurs when an electron is acquired by a neutral atom.

c)

The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

d)

How close an atom is to its neighboring atom.

81.

Which element has the smallest atomic radius?

a)

magnesium

b)

chlorine

c)

bromine

d)

argon

82.

What does the atomic radius increase down a group?

a)

There are more electrons and energy levels.

b)

There are fewer electrons and energy levels.

c)

There are more protons that need more energy levels.

d)

There are more neutrons that need more energy levels.

83.

Why does the atomic radius decrease across a period?

a)

There are more protons in the nucleus that pull electrons closer.

b)

There are more electrons in the nucleus that pull protons closer.

c)

There are more protons in the nucleus that pull neutrons closer.

d)

There are more neutrons in the nucleus that pull protons closer.

84.

Light particles are called?

a)

photons

b)

protons

c)

electrons

d)

atoms

85.

Calculate the energy for a mole of photons with a frequency ( $\nu$ ) of 4.29 x 10¹⁵ s^-1.

$E_{photon}\ =h\cdot\nu\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ 1\ mole=6.02\times10^{23}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ h\ =6.626\times10^{-34}\ J\cdot s$

a)

$1.71\times10^6\ J$

b)

$1.71\times10^{-6}\ J$

c)

171 J

d)

7.11 J

86.

What is the wavelength of light (nm) that has a frequency of 6.44 × 10¹³ s^-1 ?

$c\ =\lambda\times\nu$

c = speed of light = $3.00\times10^8\ ms^{-1}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ 1\ nm\ =\ 10^{-9}\ m$

$\lambda\ =\ wavelength\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \nu\ =\ frequency$

a)

6490 nm

b)

932 nm

c)

4660 nm

d)

6.49 × 10^-8nm

87.

The wavelength of a photon that has an energy of 6.33 × 10^-18 J is ________ m.

a)

3.79 × 10^-7

b)

3.14 × 10^-8

c)

2.38 × 10²³

d)

4.21 × 10^-24

88.

If l = 2, what are the possible m_l values?

a)

m_l= 0, 1, 2

b)

m_l = 0, 1

c)

m_l= -2, -1, 0, 1, 2

d)

m_l = -1, 0, 1

89.

If n=4, what are the possible l values?

a)

l = 0, 1, 2, 3, 4

b)

l = 0, 1, 2, 3

c)

l = -4, -3, -2, -1, 0, 1, 2, 3, 4

d)

l = -3, -2, -1, 0, 1, 2, 3

90.

What subshell does an l-value of 3 correspond to?

a)

s-subshell

b)

p-subshell

c)

d-subshell

d)

f-subshell

91.

What subshell does an l-value of 0 correspond to?

a)

s-subshell

b)

p-subshell

c)

d-subshell

d)

f-subshell

92.

How many ELECTRONS can fit within a s-subshell?

a)

2

b)

6

c)

10

d)

14

93.

How many ELECTRONS can fit within a p-subshell?

a)

2

b)

6

c)

10

d)

14

94.

How many ELECTRONS can fit within a d-subshell?

a)

2

b)

6

c)

10

d)

14

95.

How many ELECTRONS can fit within a f-subshell?

a)

2

b)

6

c)

10

d)

14

96.

How many ORBITALS does a f-subshell contain?

a)

1

b)

3

c)

5

d)

7

97.

How many ORBITALS does a d-subshell contain?

a)

1

b)

3

c)

5

d)

7

98.

How many ORBITALS does a p-subshell contain?

a)

1

b)

3

c)

5

d)

7

99.

How many ORBITALS does a s-subshell contain?

a)

1

b)

3

c)

5

d)

7

100.

Which set of Quantum numbers is not allowed

a)

(3,1,1,-1/2)

b)

(2,1,-2,+1/2)

c)

(4,2,-1,-1/2)

101.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

102.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

103.

n=4, l=3?

a)

4f

b)

4d

c)

3s

d)

3p

104.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

105.

What is the symbol for the principal quantum number?

a)

n

b)

l

c)

m_l

d)

m_s

106.

What is the symbol for the magnetic quantum number?

a)

n

b)

l

c)

m_l

d)

m_s

107.

Which of the following has an l = 0?

a)

b)

c)

d)

108.

What type of orbital is this?

a)

s

b)

p

c)

d

d)

f

109.

What type of orbital is this?

a)

s

b)

p

c)

d

d)

f

110.

What is the correct condensed electron configuration for potassium (K)?

a)

[Ar]4s¹

b)

[Kr] 4s¹

c)

[Ar] 4s²

d)

[Kr] 4s²

111.

Which of the following elements is an exception to the normal rules of electron configuration?

a)

lead (Pb)

b)

tungsten (W)

c)

iron (Fe)

d)

chromium (Cr)

112.

What is the correct condensed electron configuration for silver (Ag)?

a)

[Kr] 5s¹ 4d¹⁰

b)

[Xe] 5s¹ 4d¹⁰

c)

[Kr] 5s²4d⁹

d)

[Xe] 5s² 4d⁹

113.

What is the correct condensed electron configuration for the ion Ca²⁺?

a)

[Ar]

b)

[Ar] 4s²

c)

[Kr]

d)

[Kr] 4s²

Week 6 Exam 1 practice

Total questions: 113

Worksheet time: 3hrs 1mins

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