Free Printable ENV112 (pt3)

1.

One atomic mass unit (amu) is closest to the mass of

a)

one proton

b)

one electron

c)

the carbon-12 nucleus

d)

$6.2x10^{23}$ atoms of hydrogen

2.

How many electrons does magnesium have if it is a neutral atom?

a)

24

b)

26

c)

22

d)

48

3.

The atomic number of selenium, Se is 34, and its mass number is 79. The nucleus of Se contains

a)

34 protons and 79 neutrons

b)

34 protons and 45 neutrons

c)

45 protons and 34 neutrons

d)

34 protons, 34 electrons and 45 neutrons

4.

The total number of atoms in one formula unit of $Fe_2(SO_4)_3$ is

a)

5

b)

14

c)

15

d)

17

5.

The formula of potassium carbonate is

a)

$P_2CO_3$

b)

$K_2CO_3$

c)

$Po_2CO_3$

d)

$P_2C$

6.

What is the general outer-shell electron configuration for the halogens?

a)

$ns^6$

b)

$ns^2np^6$

c)

$ns^2np^5$

d)

$np^2$

7.

A fictional element, kryptonite (Ki) consists of two isotopes with the following abundances. What is the average atomic mass of kryptonite? Ki=285, 70.0%; Ki=289, 30.0%

a)

285 amu

b)

286 amu

c)

287 amu

d)

288 amu

8.

Which of the following electron configurations represents the electron configuration for a magnesium cation, $Mg^{2+}$ ?

a)

$1s^22s^22p^63s^2$

b)

$1s^22s^22p^63s^23p^2$

c)

$1s^22s^22p^6$

d)

$1s^22s^22p^4$

9.

Element M forms an ion $M^{2-}$ which has the same electron configuration as O (Z=8). What is the atomic number of M?

a)

Z=6

b)

Z=8

c)

Z=10

d)

Z=16

10.

What do the following elements have in common? $,^{10}Ne,^9F^-,^{12}Mg^{2+}$

a)

They are isotopes of each other

b)

They are isomers of each other

c)

They are isoelectronic with each other

d)

They are different elements so they have nothing in common

11.

Which scientist noted a definite pattern in valence numbers and arranged an early periodic table in order of the elements’ atomic mass?

a)

Enrico Fermi

b)

Dmitri Mendeleev

c)

Albert Einstein

d)

Madame Curie

12.

Which of the following is NOT a general property of the transition elements?

a)

Have high melting points

b)

Form both ionic and covalent compounds

c)

Form coloured ions

d)

Form many complex compounds

13.

Which of these elements has the highest first ionization energy?

a)

Oxygen

b)

Fluorine

c)

Carbon

d)

Sodium

14.

___ has the greatest electronegativity

a)

Si

b)

P

c)

N

d)

O

15.

___ combination of atoms can form a polar covalent bond

a)

H and H

b)

H and Br

c)

N and N

d)

Na and Br

16.

___ is an alkali metal

a)

B

b)

Mg

c)

H

d)

K

17.

An element Z has a mass number 16 and atomic number 8. What is the group number and period number of Z?

a)

Group I, Period 2

b)

Group II, Period 2

c)

Group VI, Period 2

d)

Group VI, Period 3

18.

How many moles of CO2 are present in 220 mg?

a)

5 moles

b)

0.005 mole

c)

5000 moles

d)

10 moles

19.

What is the empirical formula for a compound that contains 17.34% hydrogen and 82.66% carbon?

a)

$C_5H$

b)

$C_2H_5$

c)

$CH_3$

d)

$CH_2$

20.

What is the percent by mass of oxygen in magnesium oxide, MgO?

a)

20%

b)

40%

c)

50%

d)

60%

21.

___ is the MOST concentrated

a)

1 mole of solute dissolved in 1 liter of solution

b)

2 moles of solute dissolved in 3 liters of solution

c)

6 moles of solute dissolved in 4 liters of solution

d)

4 moles of solute dissolved in 8 liters of solution

22.

What is the total number of moles of hydrogen gas contained in $9.03x10^{23}$ ?

a)

1.50 moles

b)

2.00 moles

c)

6.02 moles

d)

9.03 moles

23.

0.372 mole of a compound has a mass of 0.152 kg. What is its molar mass?

a)

408.6 g/mol

b)

204.3 g/mol

c)

56.5 g/mol

d)

113.1 g/mol

24.

What volume of 8 M HCl is needed to prepare 1500 ml of 0.2 M HCl solution?

a)

3.75 ml

b)

140 ml

c)

28.3 ml

d)

37.5 ml

ENV112 (pt3)

Total questions: 24

Worksheet time: 12mins

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