Free Printable REVIEW 4-5

1.

Write/Draw the correct isotopic notation for this atom based on these clues:

Nickel, mass number 58, charge +2

2.

The top number in this isotope notation is

a)

the mass number

b)

the atomic number

c)

the atomic mass

d)

the neutron number

3.

Which of the following is the proper equation for determining the number of neutrons for a given isotope?

a)

mass # - atomic #

b)

atomic mass - protons

c)

protons + electrons

d)

mass # + protons

4.

Atomic number=

a)

number of neutrons

b)

atomic mass

c)

protons

d)

electrons+protons

5.

Which subatomic particle is used to identify the atom, as it never changes?

a)

protons

b)

neutrons

c)

electrons

6.

How many electrons are found in the following ion?

a)

3

b)

7

c)

10

d)

14

7.

How many neutrons are in the following isotope?

a)

108

b)

47

c)

61

d)

155

8.

How many electrons does the following have?

a)

2

b)

22

c)

10

d)

12

9.

Rubidium has two common isotopes, ⁸⁵Rb and ⁸⁷Rb. If the abundance of ⁸⁵Rb is 72.2% and the abundance of ⁸⁷Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

10.

An unknown element has three isotopes. Given the abundances and relative masses, determine (from the periodic table) which element it is.

Abundances | Relative masses

0.005% | 234.04 amu

0.720% | 235.04 amu

99.275% | 238.05 amu

HINT: You do NOT need to calculate anything here.

a)

Uranium (#92, Atomic Mass: 238.03 amu)

b)

Fluorine (#9, Atomic Mass: 19.00 amu)

c)

Mercury (#89, Atomic Mass: 200.59 amu)

d)

Polonium (#84 209 amu)

11.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

12.

How many electrons can the d sublevel hold?

a)

14

b)

10

c)

2

d)

6

13.

Choose the correct short electronic configuration for iodine.

a)

[Ar]4s²4d¹⁰4p⁵

b)

[Kr]5s²4d¹⁰5p⁵

c)

[Xe]5s²5d¹⁰5p⁵

d)

none of the above

14.

What electron configuration matches an oxygen ion (O^2-)?

a)

1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶4s²3d¹

15.

An aluminium ion (Al³⁺) would have which electron configuration?

a)

1s² 2s² 2p⁶ 3s²

b)

1s² 2s² 2p⁶ 3s² 3p¹

c)

1s² 2s² 2p⁶ 3s² 3p⁶

d)

1s² 2s² 2p⁶

16.

How are groups/families organized on the periodic table?

a)

Horizontally

b)

Vertically

c)

Diagonally

d)

From left to right

17.

What is the name given to each horizontal row on the periodic table?

a)

Families

b)

Groups

c)

Periods

d)

Rows

18.

Which is true?

a)

Cations are bigger than Anions

b)

Anions are bigger than Cations

c)

Cations and Anions are the same size.

d)

It depends upon their position on the Periodic Table

19.

Which physical property of elements is represented by y on the graph below?

a)

Ionization energy

b)

Ionic radius

c)

Atomic radius

d)

Electronegativity

20.

How many valence electrons are every atom trying to obtain?

a)

2

b)

4

c)

6

d)

8

21.

Which of these is correct?

a)

b)

c)

22.

How many valence electrons are in the following configuration?

1s² 2s² 2p⁶ 3s²

a)

6

b)

8

c)

2

d)

12

23.

How many neutrons are in Argon?

a)

18

b)

40

c)

58

d)

22

24.

Circle the location of the valence electrons of this atom. What element includes this atom? (Write the chemical symbol for the element underneath it electron configuration.)

25.

Which of the following is written correctly?

a)

A

b)

B

c)

C

d)

D

26.

What ion would be made from this atom of this element during bonding?

In order to answer this question, draw the Lewis Dot Diagram for the neutral atom AND for the ion that would be created during bonding.

27.

What is the equivalent of the molar mass of an element?

a)

Average atomic mass (from the periodic table)

b)

Atomic number (from the periodic table)

c)

Oxidation number

d)

Valence electrons

28.

What is the derived unit used for molar mass?

a)

mass/density

b)

grams/mole

c)

mass/volume

d)

moles/gram

29.

1 mole of anything is equal to:

a)

6.02

b)

6.02 x 10²³

c)

12

d)

12.602 x 10²³

30.

Which of the following has the most atoms?

a)

1 mole of oxygen

b)

1 mole of carbon

c)

1 mole of iron

d)

These all have the same number of atoms

31.

How many moles of carbon atoms are there in 5g of carbon?

a)

60 mol

b)

17 mol

c)

0.42 mol

d)

7 mol

32.

Which of the following dimensional analysis setups will correctly convert 27.76 g of Li to atoms of Li?

a)

A

b)

B

c)

C

d)

D

33.

(Hint: write out how you would solve the problem first on paper before choosing an answer.)

How would you set up the problem: if you have a sample of 2.50 g of sodium (Na), how many moles of Na do you have?

a)

$2.50g\ Na\ \times\frac{22.99\ mol\ Na}{1\ g\ Na}=$

b)

$2.50\ g\ Na\ \times\frac{1\ mol\ Na}{22.99\ g\ Na}=$

c)

$2.50\ g\ Na\ \times\frac{22.99\ g\ Na}{1\ mol\ Na}=$

d)

$2.50\ g\ Na\ \times\frac{1\ g\ Na\ }{22.99\ mol\ Na}=$

34.

How would you set up this problem: At STP, 2.5 moles of helium gas will have what volume?

a)

$2.5\ mol\ He\times\frac{22.4\ L}{mol}$

b)

$2.5\ mol\ He\times\frac{mol}{22.4\ L}$

c)

$2.5\ mol\ He\times\frac{6.022\ \times10^{23}atoms}{L}$

d)

$2.5\ mol\ He\times\frac{L}{6.022\ \times10^{23}atoms}$

35.

How would you set up this problem to solve it?

An average breath contains 500 mL of gas. Assuming the air is an ideal gas at STP, how many moles of air are pushed out with each breath?

a)

$0.500\ mL\times\frac{1L}{10^3mL}\times\frac{6.022\times10^{23}mol}{L}$

b)

$0.500\ mL\times\frac{1L}{10^3mL}\times\frac{mol}{22.4\ L}$

c)

$0.500\ mL\times\frac{1L}{10^3mL}\times\frac{22.4\ mol}{L}$

REVIEW 4-5

Total questions: 35

Worksheet time: 1hrs 6mins

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