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Chemistry 11th Ch 1-6

Total questions: 100

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

Find the molar mass of: NH3

a)

78g/mol

b)

17g/mol

c)

56g/mol

d)

25g/mol

2.

Find the molar mass of: CS2

a)

212g/mol

b)

120g/mol

c)

15g/mol

d)

76g/mol

3.

Find the molar mass of: KBr

a)

145g/mol

b)

119g/mol

c)

85g/mol

d)

52g/mol

4.

The atomic mass of Silver is: 107.87

a)

true

b)

false

5.

The atomic mass of Cesium is: 132.91

a)

true

b)

false

6.

Find the molar mass of: C2H3N

a)

124.32g/mol

b)

78.65g/mol

c)

41.053g/mol

d)

98g/mol

7.

Find the molar mass of:

CaSO4

a)

258.87g/mol

b)

189.21g/mol

c)

165.23g/mol

d)

none

8.

Which of the following defines Limiting Reactant?

a)

Consumed earlier

b)

Produces least product

c)

Both of them

9.

How many moles of H2 are required to manufacture 5 moles of NH3?

N2 + 3H2 = 2NH3

a)

2.5

b)

7.5

c)

10

d)

12.7

10.

Calculate the percent, by weight, of carbon in 154 g of C4H8O3?

a)

(a) 46%

b)

(b) 31%

c)

(c) 72%

d)

(d) 27%

e)

(e) 55%

11.

How many aluminum atoms are there in 3.50 grams of Al2O3?

a)

(a) 4.13 x 1022

b)

b) 4.90 x 1022

c)

(c) 2.07 x 1022

d)

(d) 1.68 x 1022

e)

(e) 2.45 x 1022

12.

Which of the following represents oxidation?

a)

C → CH4

b)

Fe3+ → Fe2+

c)

Cl2 → 2Cl-

d)

Zn → ZnO

13.
Which of the following molecules has hydrogen bonding?
a)
HCl
b)
HI
c)
HF
d)
HBr
14.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
15.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
16.
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
17.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
18.

Identify the Alkali Metal with the lowest mass.

a)

Lithium

b)

Potassium

c)

Calcium

d)

Helium

19.
Identify the element that is non-reactive (inert) with 4 energy levels.
a)
Krypton
b)
Argon
c)
Potassium
d)
Calcium
20.

_____ are assigned zero electronegativity.

a)

Halogens

b)

Noble gases

c)

Chalcogens

d)

Actinides

21.

Pauling assigned arbitrary value of electronegativity for _____ and _____ to calculate the electronegativity values of other elements.

a)

Sodium & Helium

b)

Nitrogen & Oxygen

c)

Hydrogen & Fluorine

d)

Beryllium & Boron

22.

. _____ values play an important role in predicting the nature of the bond.

a)

Electronegativity

b)

Electron affinity

c)

Ionisation energy

d)

Ionic radius

23.

Among halogens, which is the most electronegative element ?

a)

Iodine

b)

Bromine

c)

Chlorine

d)

Fluorine

24.

Except _____ and _____ group, all other p-block elements follow the expected trend in electronegativity.

a)

13th and 14th

b)

10th and 11th

c)

17th and 18th

d)

1st and 2nd

25.

Which of the following trend is similar to electronegativity?

a)

Atomic radius

b)

Ionic radius

c)

Ionization energy

d)

All of the choices

26.

Im the first in the periodic table.

a)

Hydrogen

b)

Helium

c)

Aluminium

d)

Magnesium

27.

My electron arrangement is 2.8.8.2

a)

Carbon

b)

Oxygen

c)

Hydrogen

d)

Nitrogen

28.

Proton number of 16.

a)

Sulphur

b)

Silicon

c)

Chlorine

d)

Phosphorus

29.

Proton number of Argon.

a)

15

b)

19

c)

18

d)

16

30.
Which of the following is the atomic number of an alkali metal?
a)
31
b)
20
c)
18
d)
19
31.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
32.

Which group does NOT have electronegativities?

a)

Alkali Metals

b)

Halogens

c)

Noble Gases

d)

Alkali Earth Metals

33.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
34.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
35.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
36.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
37.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
38.

Which atom is smaller?

a)

Ca

b)

Ca+2

39.

Which atom is larger

a)

Br

b)

Br-1

40.
Which of the following is the atomic number of an alkali metal?
a)
31
b)
20
c)
18
d)
19
41.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
42.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
43.

Which group does NOT have electronegativities?

a)

Alkali Metals

b)

Halogens

c)

Noble Gases

d)

Alkali Earth Metals

44.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
45.

This family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

46.

Sulfur is a...

a)

metal

b)

nonmetal

c)

metalloid

47.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
48.

What charge does Nitrogen typically form?

a)

-5

b)

-3

c)

+3

d)

+/-4

49.

What is the most reactive halogen?

a)

F

b)

Ts

c)

Fr

d)

Li

50.

How was the first periodic table organized?

a)

Atomic number

b)

Atomic mass

c)

Number of neutrons

51.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
52.
The outer most negatively charged particles of an atom are known as what?
a)
electrons
b)
protons
c)
neutrons
d)
valance electrons
53.

An ion is a(n)

a)

atom with a charge

b)

atom that is bonded

c)

atom that got destroyed

d)

half the distance from the bonded nuclei of two identical atoms

54.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
55.
[Ne]3s23p1 is the noble gas configuration for which element?
a)
scandium
b)
boron
c)
nitrogen
d)
aluminum
56.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
57.

What atom matches this electron configuration?

[Xe] 6s24f145d9

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

58.

There are __ energy levels

a)

1

b)

2

c)

7

d)

8

59.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
60.

what type of mixture can be separated using the arrangement shown?

a)

salt dissolved in water

b)

ink components

c)

saw dust and iron fillings

d)

sand mixed with water

61.

in this type of arrangement the substance that remains in the filter paper in the funnel is called?

a)

filtrate

b)

mixture

c)

residue

d)

dirty

62.

in this type of arrangement the substance that is obtained in the conical flask is called?

a)

water

b)

residue

c)

filtrate

d)

mixture

63.

How many cm3 is present in 1dm3?

a)

10

b)

100

c)

1000

d)

10000

64.
You know 1000 mg = 1 g.  Convert 2.5 grams into milligrams.
a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
65.
What happens when the motion of particles slows?
a)
The particles split.
b)
The particles move further apart.
c)
The particles move closer together
d)
The particles no longer move randomly.
66.

Changing from a liquid to a gas

a)

condensation

b)

vaporization

c)

sublimation

d)

melting

67.

Changing from a gas to a liquid

a)

condensation

b)

vaporization

c)

sublimation

d)

melting

68.

Changing directly from a solid to a gas

a)

condensation

b)

vaporization

c)

sublimation

d)

melting

69.

Deposition is a change from a __________

a)

gas to a solid.

b)

solid to a gas.

c)

liquid to a gas.

d)

gas to a liquid.

70.

Solid particles are able to...

a)

Move around

b)

Move in random directions

c)

Vibrate in a fixed position

d)

Be compressed

71.

A substance's _____________________ is when it changes from a solid to a liquid

a)

boiling point

b)

freezing point

c)

melting point

d)

triangle point

72.

The energy an object has due to its motion

a)

thermal energy

b)

potential energy

c)

kinetic energy

d)

gravitational energy

73.

What is a subatomic particle with a positive charge that is in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

74.

What is a subatomic particle with a negative charge? It is found in the electron cloud surrounding the nucleus.

a)

neutron

b)

proton

c)

electron

d)

electron cloud

75.

What is the combined mass of all the protons and neutrons of an atom and is approximately equal to the number of protons and neutrons?

a)

atomic mass

b)

atomic number

c)

subatomic particles

d)

nucleus weight

76.
What is true about an atom?
a)
Most of the space in an atom is taken up by the nucleus
b)
Atoms are mostly empty space
c)
Atoms have no mass
d)
Electrons have much more mass that protons or neutrons.
77.
The term "neutral" means
a)
having only a little bit of charge
b)
having a positive charge
c)
having a negative charge
d)
having no charge at all
78.

Atoms of the same element must always have the same number of

a)

Electrons

b)

Isotopes

c)

Neutrons

d)

Protons

79.

An atom's electronegativity depends on

a)

Nuclear charge

b)

Atomic radius

c)

Electron shielding

d)

All of these

80.

The separation of the positive and negative charges in a molecule is called a

a)

Pole

b)

Charge

c)

Dipole

d)

Magnet

81.

There are three types of intermolecular force: rank them from weakest to strongest

a)

van der waals, dipole-dipole, hydrogen bonding

b)

hydrogen bonding, van der waals, dipole-dipole

c)

dipole-dipole, hydrogen bonding, van der waals,

d)

dipole-dipole, van der waals, hydrogen bonding

82.

Dipole-dipole forces are:

a)

Vectors

b)

Determine the polarity of a molecule

c)

Occur in covalent molecules

d)

All of these

83.

Van der waals forces are found between

a)

Non polar molecules

b)

Polar molecules

c)

Ionic compounds

d)

Atoms

84.

Hydrogen bonding only takes place between hydrogen and

a)

Carbon, oxygen, fluorine

b)

Carbon, nitrogen, chlorine

c)

Nitrogen, oxygen, fluorine

d)

Carbon, nitrogen, fluorine

85.

What happens by changing the number of neutrons?

a)

The atomic mass changes

b)

The number of electrons changes

c)

The atomic number changes

d)

The number of protons changes

86.

What will be the molarity of a solution, which contains 5.85 g of NaCl(s) per

500 mL?

a)

4

b)

20

c)

0.2

d)

2

87.

The number of atoms present in one mole of an element is equal to Avogadro

number. Which of the following element contains the greatest number of

atoms?

a)

4g He

b)

46g Na

c)

0.4g Ca

d)

12g He

88.

What is the mass percent of carbon in carbon dioxide?

a)

40

b)

27

c)

32

d)

10

89.

Which is used to Express amount of mercury vapour in atmosphere

a)

M

b)

m

c)

Mole fraction

d)

ppm

90.

1 mole = ?

a)

60.23 x 1023

b)

6.23 x 1023

c)

6.023 x 1023

91.

The mass of 100 molecules of sucrose (C12H22O11) is_________.

a)

100 g

b)

342 g

c)

3.88 × 10–20 g

d)

5.68 × 10–20 g

92.

Number of atoms in 52 g of He are:

a)

2.865 X 1023

b)

7.83 X 1024

c)

6.023 X 1023

d)

5000

93.

How many moles of methane are required to produce 22g of CO2(g) after combustion ?

a)

2 Moles

b)

1 Moles

c)

0.5 Moles

d)

0.05 Moles

94.

A solution is 25% water, 25% ethanol and 50% acetic acid by mass. The mole fraction of water is:

a)

0.6

b)

0.856

c)

0.99

d)

0.502

95.

Which of the following statement is INCORRECT

a)

protium has no neutron

b)

C14 is used for finding age of old wooden objects

c)

Ca-40 and Ar-50 are isotopes

d)

Ca-40 and Ar -40 are isobars

96.

The number of atoms present in one mole of an element is equal to Avogadro

number. Which of the following element contains the greatest number of

atoms?

a)

4g He

b)

46g Na

c)

0.4g Ca

d)

12g He

97.

The empirical formula and molecular mass of a compound are CH2O and

180 g respectively. What will be the molecular formula of the compound?

a)

C2H4O2

b)

HCHO

c)

C6H12O6

d)

CH3COOH

98.

What will be the molarity of a solution, which contains 5.85 g of NaCl(s) per

500 mL?

a)

4

b)

20

c)

0.2

d)

2

99.

Jacques Alexandre Charles performed an experiment in a balloon, hot water, and cold water. Which of the following statements is proposed in Charles’ Law?

a)

The Kelvin temperature and the volume of a gas are directly related at constant pressure.

b)

The pressure of a fixed amount of a gas is directly proportional to the absolute temperature (Kelvin).

c)

The volume of a given mass of gas held at constant temperature is inversely proportional to its pressure.

d)

The volume of a gas varies directly with the number of moles and absolute temperature and inversely proportional with pressure.

100.

Application of Charles’ Law can be seen as one flies in a hot air balloon, when heated, causes the air to expand; thus, becomes lighter and so it rises. Which of the following is another application of Charles’ Law?

a)

A flat tire takes up less volume than an inflated tire.

b)

An inflated balloon shrinks when placed inside the refrigerator.

c)

A helium-filled balloon weights much less than an identical balloon filled with air.

d)

A syringe plunger being pressed down to draw out the fluid causes the volume inside the syringe to decrease while increasing pressure inside.

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