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Unit 3 Test Review

Total questions: 60

Worksheet time: 15hrs 0mins

Name
Class
Date
1.

The modern periodic table is arranged by ___________________.

a)

atomic number

b)

atomic mass

c)

neutrons only

d)

none of the above

2.

Match the following

a)
1.

Group

b)
2.

Period

c)

1969 Periodic Table was organized by:

3.

Atomic Mass

d)

Modern Periodic Table is organized by:

4.

Atomic Number

3.

Alkali Metals are..

a)

in group 1 and are the most reactive metals.

b)

in group 2 and are the second most reactive metals.

c)

in group 17 and are the most reactive nonmetals.

d)

in group 18 and are inert (unreactive).

4.

Alkaline Earth Metals are..

a)

in group 1 and are the most reactive metals.

b)

in group 2 and are the second most reactive metals.

c)

in group 17 and are the most reactive nonmetals.

d)

in group 18 and are inert (unreactive).

5.

Match the following

a)

in group 1 and are the most reactive metals.

1.

Alkali Metals

b)

In group 1 and are the most reactive metals.

2.

Alkaline Earth Metals

c)

In group 17 and are the most reactive nonmetals..

3.

Halogents

d)

Complete, Stable!

4.

Noble Gases

e)

Metallic elements that have valence electrons in two shells instead of only one.

5.

Transition Metals

6.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
7.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
8.
Atomic Radius is...
a)
the relative size of the atom's nucleus
b)
the relative size of the atom's electron cloud
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
9.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
10.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
11.

Which ion has the largest radius?

a)

Ga3+

b)

K+

c)

Ca2+

d)

Cl-

e)

S2-

12.

Which atom has the largest radius?

a)

Ga3+

b)

K+

c)

Ca

d)

Cl-

e)

S2-

13.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
14.

Ionization energy is the _____ energy required to _______  one mole of electron from one mole of gaseous atom at ground state.

a)

maximum, remove

b)

minimum, remove

c)

maximum, add

d)

minimum, add

15.

Across a period, Ionization energy ____a____

Down a group, ionisation energy ____b_____

a)

a : increase

b: decrease

b)

a : increase

b: increase

c)

a : decrease

b: decrease

16.

Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?

a)

Aluminum (Al)

b)

Chlorine (Cl)

17.
Which element has the greater ionization energy?
a)
Strontium
b)
Boron
18.

Which of the following factors will affect ionization energy:

a)

Atomic radius

b)

Effective nuclear charge

c)

Shielding effect

d)

All of the above

19.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size
20.

Which is larger

a)

Na

b)

Na+

21.

Which is larger

a)

I

b)

I-

22.

Which ion is larger

a)

Cu+

b)

Cu2+

23.
Why are cations larger and anions smaller than their respective atoms?
a)
Cations are larger than their respective atoms because of decreased electron repulsion
b)
Cations are larger than their respective atoms because of increased electron repulsion
c)
Anions are smaller than their respective atoms because of increased effective nuclear charge
24.
Why does ionic radius increase as you move down a group?
a)
because there are no charged atoms.
b)
because the protons and electrons cancel each other's charges.
c)
because there is more nuclear charge between protons and electrons.
25.

How does Linus Pauling define electronegativity?

a)

The ability of an atom to attract other atoms to itself

b)

The quantity of energy required for an atom to discharge an electron

c)

Linus Pauling never defined electronegativity

d)

The ability of an atom to attract electrons to itself

26.
Which has the greater EN: 
N or C?
a)
C
b)
N
27.
Which has the greater EN: 
H or F?
a)
H
b)
F
28.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

29.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

30.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

31.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
32.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

33.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

34.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

35.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

36.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

37.

What two types of atoms make a covalent bond?

a)

2 non-metals

b)

1 metal and 1 non-metal

c)

2 metals

38.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

39.

Identify the following compound as ionic or covalent: Ca(OH)2

a)

ionic

b)

covalent

40.

When naming covalent compounds,

a)

roman numerals are needed but no prefixes required

b)

both roman numerals or prefixes are not required

c)

both roman numerals and prefixes must be included

d)

prefixes are needed but roman numerals are not required

41.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
42.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
43.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
44.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
45.
A covalent compound made of one sulfur and two oxygen atoms would be named
a)
sulfur dioxide.
b)
sulfur oxide.
c)
disulfur oxide.
d)
sulfide oxygen.
46.

Select the correct formula for the

COVALENT COMPOUND

diphosphorus trioxide

a)

PO

b)

P3O2

c)

PO2

d)

P2O3

47.
Which statement explains why ethene does not dissolve in water?
a)
Ethene is polar and water is nonpolar.
b)
Ethene is nonpolar and water is nonpolar.
c)
Ethene is polar and water is polar.
d)
Ethene is nonpolar and water is polar.
48.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
49.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

50.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

51.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

52.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

53.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

54.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

55.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

56.

A ______ is made up of a single atom.

a)

monatomic

b)

polyatomic

c)

atomic

d)

element

57.

A _____ ion is a covalently bonded group of atoms with an overall positive or negative charge.

a)

monatomic

b)

polyatomic

c)

compound

d)

element

58.

Match the following

a)

Na +1

1.

Sodium Ion

b)

BrO3 -1

2.

Bromate Ion

c)

OH -1

3.

Hydroxide Ion

d)

Cl -1

4.

chloride ion

59.

MgO- name?

a)

oxygen magnesium

b)

magnesium oxide

c)

magnesium oxate

d)

magnesium oxygenate

60.

LiOH- name?

a)

hydrogen lithium

b)

lithium oxyhydride

c)

lithium oxide

d)

lithium hydroxide

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