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Chapter 2 chem review

Total questions: 47

Worksheet time: 49mins

Name
Class
Date
1.

How many protons, neutrons, and electrons are in Oxygen?

a)

Protons = 8; Neutrons = 16; Electrons = 8

b)

Protons = 8; Neutrons = 8; Electrons = 8

c)

Protons = 16; Neutrons = 8; Electrons = 16

d)

Protons = 16; Neutrons = 24; Electrons = 16

2.

Which of the following elements would have similar properties to Be

a)

S

b)

O

c)

Cl

d)

Mg

3.

What is this group on the periodic table

a)

Halogens

b)

Alkali metals

c)

Transition metals

d)

Noble gasses

4.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
5.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
6.

We know when a period ends because

a)

The elements in the row no longer have similar characteristics with each other

b)

we get to 8 valence electrons then the next period starts with 1

c)

We get to 1 valence electron then the next period starts with 8

d)

We reach 9 valence electrons and the pattern starts again with 1

7.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

lose 1 electron

b)

gain 7 electrons

8.

What two types of atoms make a covalent bond?

a)

metal atom and metal atom

b)

metal atom and non metal non atom

c)

non metal atom and non metal atom

9.

When an atom loses an electron, it becomes a _________.

a)

noble gas

b)

anion

c)

cation

10.
Write the correct formula for an ionic compound formed from S2- and Rb1+.
a)
SRb2
b)
SRb
c)
Rb2S
d)
RbS2
11.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

12.

What is the best definition of valence electrons?

a)

The outermost electron NOT involved in chemical reactions

b)

The innermost electrons involved in chemical reactions

c)

The outermost electrons involved in chemical reactions.

d)

The innermost electrons NOT involved in chemical reactions

13.

Which of the following groups/categories are likely to form cations

a)

Halogens

b)

metals

c)

nonmetals

d)

noble gases

14.

Which group of the periodic table is composed of inert (not reactive) gases?

answer choices

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

15.

Name this group: These metals are the most reactive.

a)
b)
c)
d)
16.

Why do alkali metals bond with halogens

a)

alkali metals want to gain 7 electrons halogens want to lose 7 electrons

b)

alkali metals want to gain 1 electron, halogens want to lose 1 electron

c)

alkali metals want to lose 1 electron, halogens want to gain 1 electron

d)

alkali metals want to lose 7 electrons halogens want to gain 7 electrons

17.

What did Rutherford discover about atoms?

a)

An atom is always negatively charged.

b)

An atom is mostly empty space, but has a dense positively charged center(nucleus).

c)

An atom is always positively charged.

d)

All particles will pass straight through gold foil with no change in path.

18.

Who discovered the Electron?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Erwin Schrodinger

d)

Niels Bohr

19.

Who created this model?

Plum Pudding Model

a)

JJ Thomson

b)

Ernest Rutherford

c)

John Dalton

d)

James Chadwick

20.

Who used the Cathode Ray Tube?

a)

JJ Thomson

b)

Ernest Rutherford

c)

Erwin Schrodinger

d)

Niels Bohr

21.

The law of definite proportions states that a given chemical compound always contains the same _ in the exact same _ by mass.

a)

elements, compounds

b)

elements, molecules

c)

elements, proportions

d)

proportions, elements

22.

The percentage of copper and oxygen in samples of “CuO” obtained by different methods were found to be the same. This illustrates the law of:

a)

Definite proportions

b)

Conservation of mass

c)

Multiple proportions

d)

Reciprocal proportions

23.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
24.

Write the formula for barium + nitrogen

a)

Ba2N3

b)

Ba3N2

c)

BaN

d)

BaN3

25.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
26.

Formula for lead (II) chloride

a)

PbCl2

b)

Pb2Cl

c)

Pb2Cl3

d)

Pb3Cl2

27.

Formula for Disilicon Heptasulfide

a)

SiS6

b)

SiS7

c)

Si2S6

d)

Si2S7

28.

Name for CO

a)

carbon monoxide

b)

carbon oxide

c)

monocarbon oxide

d)

carbide monoxide

29.
What is the proper name for CaCl2?
a)
Calcium dichloride
b)
Monocalcium dichloride
c)
Calcium chloride
d)
Calcium chlorine
30.

H2SO4

a)

-ide

b)

-ate

31.

What is the name for SiCl4?

a)

silicon tetrachloride

b)

silicon quadchloride

c)

monosilicon tetrachloride

d)

silicon chloride

32.

What is the formula for copper(I) sulfate?

a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

33.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
34.

What is the correct formula for Calcium Phosphate?

a)

Ca3(PO4)2

b)

Ca3(PO4)

c)

Ca2(PO4)

d)

Ca2(PO4)2

35.

What is the name for the compound with the formula NH4Cl

a)

ammonium chloride

b)

ammonium hypochlorite

c)

ammonium hypochlorate

d)

ammonium chlorate

36.

What is the correct formula for aluminum nitrate

a)

Al2(NO3)3

b)

Al(NO3)3

c)

Al(NO3)2

d)

Al2(NO3)4

37.

What is the proper formula for copper II bromide?

a)

CuBr

b)

CuBr2

c)

Cu2Br

38.
Name the compound using appropriate rules:
FeCl3
a)
Chloride Iron
b)
Iron III Chloride
c)
Chloride III Iron
d)
I have no clue
39.

What is the name of the following formula: Cu3N

a)

copper nitride

b)

copper (iii) nitride

c)

copper (i) nitride

d)

copper (iii) nitrogen (i)

40.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
41.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
42.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
43.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
44.

Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37, The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant?

a)

Cl-35

b)

Cl-37

c)

Cannot be determined from the information provided.

45.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
46.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
47.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron

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