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CHAPTER 1,2,3,4 REVISION EOT SYLLABUS pages from 14-125

Total questions: 155

Worksheet time: 3hrs 4mins

Name
Class
Date
1.

This shape is that of

a)

s-orbital

b)

d-orbital

c)

p-orbital

d)

f-orbital

2.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

3.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

4.

n represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

5.

How is an orbital is defined in the quantum mechanical model of the atom?

a)

circular path traveled by a proton around an orbital

b)

circular path traveled by an electron around an orbital

c)

region of the most probable proton location

d)

region of the most probable electron location

6.

How many orbitals are there with principal quantum number n=4?

a)

1

b)

4

c)

9

d)

16

7.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

8.

As the energy level goes higher, the electrons

a)

have lower in energy

b)

are more stable

c)

are weaker

d)

are farther from the nucleus

9.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

10.

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

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

11.

How many electrons are in 1s2 2s2 2p4?

a)

5

b)

6

c)

8

d)

13

12.
An electron fro which n=4 has more ____ than an electron for which n=2.
a)
spin
b)
particle nature
c)
energy
d)
wave natrue
13.
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called 
a)
d orbitals.
b)
p orbitals.
c)
f orbitals.
d)
s orbitals
14.
According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus
a)
in specific, allowed orbits.
b)
in one fixed orbit at all times.
c)
at any of an infinite number of distances, depending on its energy.
d)
counterclockwise.
15.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
16.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
17.

Which section of the spectrum is the ONLY one we can see?

a)

X-rays

b)

Gamma Rays

c)

Visible Light

d)

Ultraviolet Rays

18.

Who proposed that electrons are only found in specific, discrete circular orbits around the nucleus?

a)

Louis de Broglie

b)

Niels Bohr

c)

Werner Heisenberg

d)

Wolfgang Pauli

19.

Bohr states that when atoms absorb precise amount of energy, the electron will ...

a)

Falls into the nucleus

b)

Falls to the ground state

c)

Moves to another atom

d)

Excites to higher state of energy

20.

An emission spectrum is produced when ...

a)

electron absorbs sufficient energy

b)

electrons excites from lower to higher energy level

c)

electron falls from higher to lower energy level

d)

atoms absorbs too much energy

21.

When atom _________ energy, the electron excites to higher energy level. The electron is ________ at higher state. The electron then ________ energy by emitting light when it falls back to lower energy level

a)

absorbs, stable, absorbs

b)

absorbs, unstable, loses

c)

loses, unstable, loses

d)

loses, stable, absorbs

22.

Which of the following line spectrum series of hydrogen atom is found in ultraviolet region?

a)

Balmer series

b)

Brackett series

c)

Paschen series

d)

Lyman series

23.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

24.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

25.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
26.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
27.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
28.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
29.

No two electrons will have all the four quantum numbers identical

a)

Hunds rule

b)

Paulis exclusion principle

c)

Aufbau principle

d)

n + l rule

30.

An orbital can at most hold how many electrons?

a)

4

b)

6

c)

2

d)

1

31.

What is incorrect about this orbital diagram?

a)

Both arrows in the filled 2p box should be pointing the same direction

b)

There is nothing incorrect with this diagram

c)

In the there should only be 1 arrow in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing the same direction.

32.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
33.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
34.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
35.
What is this element? 
[Ar]4s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
36.
What is the noble gas shorthand for Sulfur?
a)
[Ar]3p4
b)
[He]3s23p4
c)
[Ne]3s23p4
d)
[Na]3s23p4
37.

How many valence electrons does this element have?

a)

2

b)

8

c)

12

d)

4

38.

Who is known as the father of periodic table, who arranged the elements in order?

a)

Dmitri Mendeleev

b)

Robert Hooke

c)

Jons Jacob Berzelius

d)

John Dalton

39.

How many periods are there in the periodic table?

a)

18 periods

b)

8 periods

c)

17 periods

d)

7 periods

40.

An atom of an element has the electronic confi-guration 2,8,2. To which group does it belong?

a)

(a) 4th group

b)

(b) 6th group

c)

(c) 3rd group

d)

(d) 2nd group

41.

The arrangement of elements in the Modem Periodic Table is based on their

a)

(a) increasing atomic mass in the period

b)

(b) increasing atomic number in the horizontal rows

c)

(c) increasing atomic number in the vertical columns

d)

(d) increasing atomic mass in the group

42.

Newlands relation is called

a)

a) Musical Law

b)

(b) Law of Octaves

c)

(c) Periodic Law

d)

(d) Atomic Mass Law

43.

[He]2s2 determine the group,period and block

a)

2,3,s

b)

2,2,s

c)

2,1,s

d)

3,2,s

44.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost orbit of an atom

45.
a)

14

b)

4

c)

3

d)

28

46.

Why do all bonds form?

a)

To fill up the outer shell.

b)

To achieve the one or duplet electronic configuration

47.

Which electron configuration belongs to a Chloride (Cl-) ion?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

48.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
49.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
50.

Which of the following is the correct abbreviated noble gas electron configuration for chlorine?

a)
[Ne]3s23p5
b)
[He]2s22p63s23p5
c)
[Mg]3p5
d)
[Ne]1s22s22p63s23p5
51.

Which would be the correct electron configuration for the Fe+4 ion?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d3

c)

1s2 2s2 2p6 3s2 3p6 3d4

d)

1s2 2s2 2p6 3s2 3p6 4s1 3d6

52.

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

53.
An ionic bond results due to the __________ attraction between 2 oppositely charged ions.
a)
delocalized
b)
weird
c)
electrostatic
d)
ionization
54.

Which of the electronic configurations of ions below that shows pseudo-noble gas configurations?

a)

As3+ : [Ar]4s23d10

b)

Mn2+ : [Ar]3d5

c)

Sn4+ : [Kr]4d10

55.

Ionic bonds involves which of the following

a)

sharing of electrons

b)

transfer of electrons

56.

Which of the following pairs is likely to form an ionic bond

a)

Oxygen and Carbon

b)

Oxygen and Oxygen

c)

Oxygen and Magnesium

d)

Oxygen and Sulfur

57.

The positive ions tend to _____________ electrons.

a)

Share

b)

Lose

c)

Gain

d)

Neutral

58.

Ionic bonds form between two ions that have...

a)

Positive Chargers

b)

negative charges

c)

Same Charges

d)

Opposite Charges

59.

How does calcium become a calcium ion?

a)

Lose 2 electrons

b)

Gain 2 electrons

c)

Lose 1 electron

d)

Gain 1 electron

60.

How does oxygen become an oxide ion?

a)

Lose 2 electrons

b)

Gain 2 electrons

c)

Lose 1 electron

d)

Gain 1 electron

61.

What is the ionic compound that is formed when you combine Li+ and N-3 ions?

a)

LiN

b)

LiN3

c)

Li3N2

d)

Li3N

62.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
63.
Which is the correct lewis dot structure for calcium chloride?
a)
A
b)
B
c)
C
64.

What is the name for the ionic compound MgCl2?

a)

magnesium chloride

b)

manganese dichloride

c)

magnesium dichloride

d)

manganese II chloride

65.

What does the blue circle represent?

a)

proton

b)

neutron

c)

electron

66.

Factors affecting the value of lattice energy

a)

the size of the ions only

b)

the charges of the ions only

c)

BOTH the size of the ions AND the charges of the ions

67.

Bond breaking is

a)

exothermic

b)

endothermic

68.

bond making is

a)

exothermic

b)

endothermic

69.

When comparing different ionic compounds, the one with the greater charges will have a _______ magnitude of lattice energy.

a)

greater

b)

less

c)

same

70.

When comparing different ionic compounds, the one with the ions of greater size or radius will have a _______ magnitude of lattice energy.

a)

greater

b)

smaller

c)

same

71.

Choose the ionic compound with the greater magnitude of lattice energy.

a)

CaCl2

b)

KCl

72.

Choose the ionic compound with the greater magnitude of lattice energy.

a)

NaCl

b)

KCl

73.

Choose the ionic compound with the greater magnitude of lattice energy.

a)

CaCl2

b)

CaS

74.

What is the correct name for the polyatomic ion below?

CO32-

a)

carbon

b)

carbide

c)

carbonate

d)

carbonite

75.

What is the correct formula for sulfate ion?

a)

SO32-

b)

SO42-

c)

SO24-

d)

SO23-

76.

What is the correct formula for the compound named "aluminum nitrate"

a)

AlNO3

b)

Al3NO3

c)

Al(NO3)3

d)

Al3(NO3)3

77.

What is the correct formula for the compound named "calcium phosphate"

a)

CaPO4

b)

Ca2(PO4)3

c)

Ca3(PO4)2

78.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
79.

The ionic compound NH4ClO4 is

key reactant used in solid rocket boosters, such

as those that power the space shuttle into orbit.

Name this compound.

a)

Ammonium perchlorate

b)

Ammonium chlorate

c)

Ammonia perchlorate

d)

Ammonium perchlorite

80.

What subscripts would you most

likely use if the following substances formed an

ionic compound? an alkali metal and a nonmetal from group 16

a)

1,1

b)

1,2

c)

2,1

d)

2,2

81.

Metallic bond is an electrostatic force between ____________ metallic ions and the sea of delocalised electrons.

a)

negative charge

b)

positive charge

c)

atom

d)

molecule

82.

What is Y?

a)

Positive ions are immersed in the sea of electrons

b)

Negative ions are immersed in the sea of electrons

c)

Molecule are immersed in the sea of electrons

d)

Atom are immersed in the sea of electrons

83.

Which one is correct diagram of metalic bond for Na?

a)

A

b)

B

84.

Physical properties of metallic bond

i-Good conductors of heat and electricity

ii-Ductile

iii-Malleable

iv-Insulator

a)

i and ii

b)

i,ii and iv

c)

i,ii and iii

d)

i,ii,iii and iv

85.

This statement is explain about which physical properties?

"metallic bond is flexible and strong which can be hammered into sheets or drawn into wires without breaking"

a)

Malleability

b)

Ductility

c)

Thermal conductivity

d)

Malleability and Ductility

86.

Metallic bond have....

a)

high electrical conductivity and high thermal conductivity

b)

low electrical conductivity and high thermal conductivity

c)

high electrical conductivity and low thermal conductivity

d)

low electrical conductivity and low thermal conductivity

87.

The delocalised ______ in metals are mobile and free to move away from a negative electrode to a positive electrode when a metal is subjected to an electrical potential

a)

protons

b)

neutrons

c)

electrons

d)

atoms

88.

Factors affecting metallic bond strength?

______________ and atomic radius

a)

number of valence electrons

b)

number of electrons

c)

number of electronic configuration

d)

number of valance protons

89.

The greater the number of delocalised

      electrons, the ______ the forces

a)

Weaker

b)

Stronger

90.

Na vs Mg vs Al

The greater the number of delocalised

      electrons, the stronger the forces, thus higher boiling point.

Which one have highest boiling point?

a)

Na

b)

Mg

c)

Al

91.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
92.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
93.
How many pi bonds does this have? 
a)
1
b)
2
c)
3
d)
4
94.
How many sigma bonds does this have? 
a)
1
b)
2
c)
3
d)
4
95.
Pi bonds are formed by 
a)
side to side overlap of s orbitals
b)
end to end overlap of s orbitals
c)
side to side overlap of p orbitals
d)
end to end overlap of p orbitals
96.
How many pi bonds does this have? 
a)
0
b)
1
c)
2
d)
3
97.
How many sigma bonds does this have? 
a)
0
b)
1
c)
2
d)
3
98.

How many sigma bonds are in the following molecule?

a)

0

b)

1

c)

2

d)

5

e)

6

99.

How many sigma bonds are in the following molecule?

a)

0

b)

4

c)

8

d)

12

e)

16

100.

Name the bond in which the orbitals overlap head to head

a)

Ionic bond

b)

sigma bond

c)

pi bond

101.

As bond length increase the strength...

a)

increases

b)

decreases

c)

no change

102.

The energy required to break the bonds between two covalently bonded atoms

a)

bond dissociation energy

b)

activation energy

c)

none of these

103.

The number of pairs of electrons shared in triple covalent bond

a)

Two

b)

Three

c)

One

104.

The smaller the bond length, ........................ is the bond dissociation energy

a)

smaller

b)

greater

c)

no change

105.

The name of P4S10 is

a)

phosphorous sulfide

b)

tetraphosphorus decasulfide

106.

What is the name of N2O5?

a)

Dinitrogen pentaoxide

b)

Nitrogen pentaoxide

107.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
108.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
109.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
110.

What is the name of PBr3

a)

phosphorus tribromide

b)

phosphorus bromide

c)

phosphorus (III) bromide

d)

phosphorus bromine

111.
Ionic compounds are bonds between
a)
Metals and Metals
b)
Metals and Nonmetals
c)
Nonmetals and Nonmetals
d)
None of the above
112.

Oxyacids will contain __________. Check all that apply.

a)

chlorine

b)

an oxoanion

c)

just hydrogen and a non-metal

d)

the O-2 ion

e)

the H+ ion

113.

The suffix -ite in the name of a polyatomic ion becomes ______ in the acid name.

a)

-ous

b)

-ate

c)

-ide

d)

-ic

114.

The suffix -ic in the name of an oxyacid, implies that the polyatomic ion in the acid has a ________ suffix.

a)

-ous

b)

-ate

c)

-ide

d)

-ite

115.

What prefix is used to name binary acids?

a)

per-

b)

hydro-

c)

hypo-

d)

bi-

116.

What is the formula for hydrobromic acid?

a)

HBrO

b)

HBrO2

c)

HBrO3

d)

HBr

117.

What anion is in phosphoric acid?

a)

PO4-3

b)

PO3-3

c)

P-3

d)

H+

118.

What is the formula for sulfuric acid?

a)

H2S

b)

HS

c)

H2SO4

d)

H2SO3

119.

Name the compound: (NH4)2S

a)

ammonium sulfide

b)

nitrogen tetrahydrogen sulfide

c)

diammounium sulfate

d)

ammonium sulfate

120.

The chemical bond formed when two atoms share electrons is call a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

electron bond

121.
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.
122.

An atom with a different number of electrons than it should have (more or less) is called an ---

a)

isotope

b)

valence electron

c)

ion

d)

octet

123.

Which Lewis Dot Structure  is correct for the particular element?

a)
b)
124.

Al2O3, LiF, BeCl2 are...

a)

ionic compounds

b)

covalent compounds

c)

metallic compounds

125.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
126.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

127.

State VSEPR Theory.

a)

The electron pairs in the valence shell surrounding a terminal atom repel one another and arrange themselves as far apart as possible to minimize the repulsion.

b)

The electron pairs in the valence shell surrounding a central atom repel one another and arrange themselves as far apart as possible to minimize the repulsion.

c)

The electron pairs in the valence shell surrounding a central atom repel one another and arrange themselves as close as possible to minimize the repulsion.

128.

Any molecule with only two atoms must be linear. Three-atom molecules such as BeCl2 can also be linear. For linear molecules, the bond angle is

a)

90°

b)

180°

c)

108°

d)

120°

129.

Which molecule would have this molecular geometry?

a)

BF3

b)

CH4

c)

PCl5

d)

CO2

130.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Linear

d)

Bent

131.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
132.

To determine the molecular geometry of a compound by using VSEPR theory, double bond and triple bonds are considered as

a)

two or three bonding pairs

b)

two bonding pairs

c)

five bonding pairs

d)

one bonding pair

133.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
134.

Why is the molecule polar?

a)

There is a non bonding pair electrons on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no non bonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

135.

Classify the above molecule.

a)

Polar

b)

Non polar

136.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
137.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
138.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
139.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
140.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
141.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

142.

Which of these atoms is the most electronegative?

a)

Bromine

b)

Fluorine

c)

Hydrogen

d)

Potassium

143.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

144.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

145.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

146.

Do noble gases have electronegativity values?

a)

yes

b)

no

147.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
148.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

149.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

150.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

151.

When you have Zn-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

152.

How would the melting point and boiling point for polar covalent bond?

a)

High

b)

Low

153.

How would the melting point and boiling point for nonpolar covalent bond?

a)

High

b)

Low

154.

What would solubility look like for polar covalent bond in water?

a)

soluable

b)

nonsoluable

155.

What would solubility look like for nonpolar covalent bond in water?

a)

soluable

b)

nonsoluable

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