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Periodic table and properties

Total questions: 100

Worksheet time: 1hrs 3mins

Name
Class
Date
1.

As you move across a row (period) on the periodic table, the atomic radius ______________________

a)

Increases

b)

Decreases

c)

Stays the same

d)

Explodes

2.

Ionization energy is the energy needed to _________ an electron.

a)

Fission

b)

Explode

c)

Remove

d)

Add

3.

As you move across a row on the periodic table, ionization energy ______________________

a)

Decreases

b)

Increases

c)

Stays the same

4.

Which group of elements has the lowest ionization energy?

a)

Group 1

b)

Group 2

c)

Group 3

d)

Group 4

5.

Group VIII A elements are called ________________

a)

Alkali metals

b)

Transition metals

c)

Halogen

d)

Noble gases

6.

Group I A elements (not including hydrogen) are called ________________

a)

Alkali metals

b)

Transition metals

c)

Halogen

d)

Noble gases

7.

Which of the following elements would have the smallest atomic radius?

a)

Li

b)

Be

c)

C

d)

Ne

8.

Which statement about subatomic particles is true?

a)

Protons, neutrons, and electrons all have about the same mass.

b)

Unlike protons or neutrons, electrons have no mass.

c)

Neutrons have no charge and no mass.

d)

An electron has far less mass than either a proton or neutron.

9.

Which element in Period 3 has the highest melting point?

a)

Silicon (Si)

b)

Germanium (Ge)

c)

Carbon (C)

d)

Argon (Ar)

10.

The number of protons in one atom of an element is that element’s

a)

mass number.

b)

balanced charge

c)

atomic number

d)

isotope

11.

To find the number of neutrons in an atom, you would subtract

a)

mass number from atomic number

b)

atomic number from mass number

c)

atomic number from electron number

d)

isotope number from atomic number

12.

Which statement is true concerning the periodic table?

a)

rows go up and down and groups go across the table

b)

groups go up and down and rows go across the table

c)

rows go up and down and groups go up and down the table

d)

rows go across the table and groups go across the table

13.

Which list of elements contains only metals?

a)

carbon, iodine, tin

b)

tin, copper, cesium

c)

helium, iron, copper

d)

iodine, carbon, argon

14.

Which statement is true about the metalloid silicon?

a)

Silicon is a better conductor of electric current than silver is.

b)

Silicon does not conduct electric current under any conditions.

c)

Silicon's ability to conduct electric current does not vary with temperature.

d)

Silicon is a better conductor of electric current than sulfur is.

15.

Group VII A of the periodic table contains the

a)

most reactive metals.

b)

most reactive nonmetals.

c)

least reactive nonmetals.

d)

least reactive metals.

16.
How are elements on the periodic table arranged by?
a)
in alphabetic order
b)
simular physical & chemical properties
c)
their symbols
d)
Just simular physical properties
17.
What element is will have the most similar physical and chemical properties to the element Sulfur (S)?
a)
Carbon (C)
b)
Phosphorous (P)
c)
Oxygen (O)
d)
Neon (Ne
18.
What element is will have the most similar physical and chemical properties to the element Lithium (Li)?
a)
Sodium (Na)
b)
Magnesium (Mg)
c)
Beryllium (Be)
d)
Calcium (Ca)
19.
What element is will have the most similar physical and chemical properties to the element Nitrogen (N)?
a)
Phosphorous (P)
b)
Carbon (C)
c)
Oxygen (O)
d)
Sulfur (S)
20.
Sodium (Na) is found in period 
a)
3
b)
2
c)
4
d)
1
21.
The atomic number tells you what?  READ THE ANSWERS CAREFULLY
a)
only the number of electrons
b)
 only the number of protons
c)
only the number of neutrons
d)
the number of both electrons and protons in an atom.
22.

A subatomic particle that has a positive charge and that is found in the nucleus of an atom

a)

Proton

b)

elecrtron

c)

groups

d)

neutrons

23.

An atom of element X has 4 shells containing electrons. When element X reacts with chlorine, a compound with formula XCl is formed. Which of the following is the element X?

a)

Calcium

b)

Potassium

c)

Sodium

d)

Silicone

24.

Table shows the arrangement of electrons of elements in Period 3 of the Periodic Table. Which one of the following shows the correct descending order of their atomic radii?

a)

M,L,N,P,K

b)

L,M,N,K,P

c)

P,K,N,M,L

d)

K,L,M,N,P

25.

The following are the uses of inert gases except

a)

used in advertising lights

b)

used to fill a weather balloons

c)

used in lasers for eye treament

d)

used as a catalyst in Haber process

26.

Sodium and rubidium are both elements in Group 1 of the Periodic Table. Which of the following statements is correct?

a)

Both metals form acidic oxides

b)

Rubidium has a lower melting point than sodium

c)

Rubidium reacts less quickly with water than sodium

d)

Rubidium has less electrons compared to sodium

27.

The different reactivity of Group 1 elements of the Periodic Table is due to the

a)

I,II,III only

b)

I,II,IV only

c)

I,III,IV only

d)

II,III,IV only

28.

Which one of the following statements best accounts for the inert properties of Group 18 elements?

a)

All of them have 18 elements in an atom

b)

All of them have 8 valence electrons in each atom

c)

All of them are rare gases and very difficult to find

d)

Their valence shell are completely filled by electrons

29.

Fluorine is the first element in Group 17 of the Periodic Table. Which statement about fluorine is not correct?

a)

It forms ionic compound with sodium

b)

It is gas at room temperature and pressure

c)

Its molecules are diatomic at room temperature

d)

Its molecules are monoatomic at room temperature

30.
These will determine what element an atom is. 
a)
number of neutrons
b)
number of electrons
c)
number of atoms 
d)
number of protons 
31.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
32.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

33.

In the modern periodic table, the period indicates the value of:

a)

Atomic number

b)

Atomic mass

c)

Principal quantum number

d)

Azimuthal quantum number.

34.

The elements which occupy the middle block (d) in the periodic table are called ................ elements.

a)

transition

b)

alkali

c)

alkaline earth

d)

noble

35.

In the periodic table, the elements which are similar in their Chemical & physical properties are located in the same ................

a)

period

b)

group

c)

nucleus

d)

energy level

36.

Choose which of the following position is correct for Neon (z = 10)

a)

Period : 2

Group : 17

p-block

b)

Period : 2

Group : 18

s-block

c)

Period : 2

Group : 18

p-block

37.

Choose the correct position for element Krypton (Z= 36)

a)

Group : 18

Period : 4

p-block

b)

Group 8

Period : 4

p-block

c)

Group: 18

Period 3

p-block

38.

Bromine has the valence electronic configuration of 4s2 3d10 4p5. Choose the correct position of Br element in Periodic Table.

a)

Group: 15

Period : 4

d-block

b)

Group: 17

Period: 4

d-block

c)

Group : 17

Period : 4

p-block

39.

In the modern periodic table the block d is

a)

Noble gases

b)

Transitional elements

c)

Metals

d)

Non-metals

40.
How many valence electrons are found in atoms of group 15?
a)
4
b)
5
c)
2
d)
3
41.

Surrounding the nucleus is a cloud-like region of moving _________________________.

a)

protons

b)

neutrons

c)

electrons

42.

A group of two or more atoms held together by chemical bonds:

a)

atom

b)

element

c)

molecule

43.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

44.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
45.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
46.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
47.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
48.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
49.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
50.

What is the atomic radius?

a)

The distance from the nucleus to the outer boundary of an atom

b)

The distance from one side of an atom to the other side

c)

The distance around the atom

d)

The distance between atoms in the gas phase

e)

The distance between atoms in the solid phase

51.

Which of the following elements would be smaller: indium or gallium?

a)

indium

b)

gallium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

52.

Which of the following elements would be larger: potassium or cesium?

a)

potassium

b)

cesium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

53.

Which of the following elements would be larger: potassium or cesium?

a)

potassium

b)

cesium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

54.

Which of the following elements would be the largest: copper, zinc, silver or cadmium?

a)

copper

b)

zinc

c)

silver

d)

cadmium

e)

cannot be determined

55.

Why is iodine larger than bromine?

a)

iodine has a greater number of electrons than bromine

b)

iodine has a greater number of protons than bromine

c)

iodine has more occupied energy levels and greater shielding than bromine

d)

iodine has more neutrons than bromine

e)

iodine has more valence electrons than bromine

56.

The definition for Ionization Energy is:

a)

The energy required to remove an electron from the outer energy level of an element in the gaseous state.

b)

A measure of the tendency of an atom to take up electrons in order to form a negative ion.

c)

The amount of energy released when an electron is added to an atom in the ground state.

57.

Why do Group 18 elements have such high Ionization Energies?

a)

They have full outer energy levels and therefore do not want to lose electrons from their outer energy level.

b)

They are non metals.

c)

They are metals

58.

Why do Group 1 elements have such low Ionization Energies?

a)

They have full outer energy levels and therefore do not want to lose electrons from their outer energy level.

b)

They are non metals and therefore require more electrons to complete their outer energy level.

c)

They are metals and its easier to give away the electrons in their outer energy level.

59.

The definition for Electron Affinity is:

a)

The energy required to remove an electron from the outer energy level of an element in the gaseous state.

b)

A measure of the tendency of an atom to take up electrons in order to form a negative ion.

c)

The amount of energy released when an electron is added to an atom in the ground state.

60.

Why is the Electron Affinity in Group 1 elements so low?

a)

They want to accept electrons

b)

They have opposite charges which repel.

c)

They do not want to accept electrons.

61.

Why is the Electron Affinity in Group 17 elements so high?

a)

They want to accept electrons

b)

They have opposite charges which repel.

c)

They do not want to accept electrons.

62.

The definition for Electronegativity is:

a)

The energy required to remove an electron from the outer energy level of an element in the gaseous state.

b)

A measure of the tendency of an atom to take up electrons in order to form a negative ion.

c)

The amount of energy released when an electron is added to an atom in the ground state.

63.

The distance between nucleus and outermost shell occupied electron

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

64.

The degree of oxidation (loss of electrons) of an atom in a chemical compound

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

65.

Atomic radii trends is . . . .

a)

generally decrease along each period of the table, from the alkali metals to the noble gases; and increase down each group.

b)

generally increase along each period of the table, from the alkali metals to the noble gases; and increase down each group.

c)

generally increase along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

d)

generally decrease along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

66.

Ionization energy trends is . . . .

a)

becomes greater up and to the right of the periodic table.

b)

becomes greater down and to the right of the periodic table.

c)

becomes greater up and to the left of the periodic table.

d)

becomes greater down and to the left of the periodic table.

67.

Electronegativity trends is . . . .

a)

increases on passing from left to right along a period, and decreases on descending a group.

b)

increases on passing from left to right along a period, and increases on descending a group.

c)

decreases on passing from left to right along a period, and decreases on descending a group.

d)

decreases on passing from left to right along a period, and increases on descending a group.

68.

Electron affinity trends is . . . .

a)

generally increases across a period, and a trend of decreasing electron affinity going down groups would be expected.

b)

generally decreases across a period, and a trend of decreasing electron affinity going down groups would be expected.

c)

generally increases across a period, and a trend of increasing electron affinity going down groups would be expected.

d)

generally decreases across a period, and a trend of increasing electron affinity going down groups would be expected.

69.

Metallic character trends is . . . .

a)

decrease going across a period and tends to increase going down a group.

b)

increase going across a period and tends to increase going down a group.

c)

decrease going across a period and tends to decrease going down a group.

d)

increase going across a period and tends to decrease going down a group.

70.

Which element has bigger atomic radii?

a)

Beryllium is bigger than Fluorine

b)

Oxygen is bigger than Sulphur

c)

Litihium is bigger than Sodium

d)

Phosphorus is bigger than Bromine

71.

Which element has smaller atomic radii?

a)

Beryllium is smaller than Fluorine

b)

Sulphur is smaller than Oxygen

c)

Litihium is smaller than Sodium

d)

Potassium is smaller than Bromine

72.

Which element has higher ionization energy?

a)

Chlorine is higher than Sodium

b)

Phosphorus is higher than Nitrogen

c)

Silicon is higher than Carbon

d)

Magnesium is higher than Aluminium

73.

Which element has lower ionization energy?

a)

Chlorine is lower than Sodium

b)

Phosphorus is lower than Nitrogen

c)

Carbon is lower than Silicon

d)

Aluminium is lower than Magnesium

74.

Which element has higher electronegativity?

a)

Fluorine is higher than Oxygen

b)

Potassium is higher than Sodium

c)

Aluminium is higher than Boron

d)

Phosphorus is higher than Chlorine

75.

Which element has lower electronegativity?

a)

Fluorine is lower than Oxygen

b)

Potassium is lower than Sodium

c)

Boron is lower than Aluminium

d)

Chlorine is lower than Phosphorus

76.

Which element has higher electron affinity?

a)

Bromine is higher than Calsium

b)

Chlorine is higher than Fluorine

c)

Magnesium is higher than Beryllium

d)

Sodium is higher than Aluminium

77.

Which element has lower electron affinity?

a)

Bromine is lower than Calsium

b)

Chlorine is lower than Fluorine

c)

Berylliumis lower than Magnesium

d)

Aluminium is lower than Sodium

78.

Which element is more metallic?

a)

Sodium is more metallic than Aluminium

b)

Fluorine is more metallic than Beryllium

c)

Potassium is more metallic than Lithium

d)

Chlorine is more metallic than Silicon

79.

For which of the following transformations does the reactive carbon undergo a change in hybridization?

a)

methane to chloromethane

b)

methanol to methanal

c)

methanal to methanoic acid

d)

chloromethane to methanol

80.

Which molecule does not act as a nucleophile in a reaction with a halogenoalkane?

a)

Water

b)

Ethanol

c)

Hydroxide ion

d)

Ammonium ion

81.

Which compounds reacts fastest with water?

a)

(CH3)3CBr

b)

(CH3)3CCl

c)

CH3CH2CH2CH2Br

d)

CH3CH2CH2CH2Cl

82.

The reaction between 2-chloro-2-methylpropane, (CH3)3CCl, and aqueous sodium hydroxide is an example of

a)

Unimolecular nucleophilic addition

b)

Bimolecular nucleophilic addition

c)

Unimolecular nucleophilic substitution

d)

Bimolecular nucleophilic substitution

83.

Which statement about the reactions of halogenoalkanes with aqueous sodium hydroxide is correct?

a)

Primary halogenoalkanes react mainly by SN1 mechanism.

b)

Chloroalkanes react faster than iodoalkanes.

c)

Tertiary halogenoalkanes react faster than primary halogenoalkanes.

d)

The rate of an SN1 reaction depends on the concentration of aqueous hydroxide.

84.

Which of the chloroalkanes below will hydrolyse most rapidly?


a)

CH3CH2CH2CH2Cl

b)

CH3CH(CH3)CH2Cl

c)

CH3CH2CHClCH3

d)

(CH3)2CClCH2Cl

85.

Which substance(s) is(are) most likely to react with hydroxide ions by means of a SN2 mechanism?

I. C6H5Cl

II. (CH3)3CCl

III. (CH3)2CHCH2Cl

IV. CH3CH2CH2CH2Cl

a)

I and III

b)

I and IV

c)

III and IV

d)

I, III and IV

86.

Which statement is incorrect regarding the reaction of ammonia with alkyl halides?

a)

This is a Lewis acid base reaction

b)

Ammonia acts as a nucleophile and forms dative bond with the carbon

c)

The product of the reaction is an amine

d)

The hybridisation of the carbon atom that receives the ammonia molecule changes from sp3 to sp2

87.
Which of the following statement is FALSE about nucleophile?
a)
It is a lone pair donor
b)
It is a Lewis base
c)
Attracted to electron deficient carbon
d)
It must be a negatively charged ions
88.
The type of reaction shown is called
a)
Addition reaction
b)
Nucleophilic reaction
c)
Electrophilic reaction
d)
Substitution reaction
89.
SN2 reaction is favoured by
a)
1° halogenoalkane
b)
2° halogenoalkane
c)
3° halogenoalkane
d)
1° and 2° halogenoalkane
90.
Which of the following statements applies to the E2 mechanism?
a)
It occurs with inversion of stereochemistry
b)
It occurs with racemization
c)
It proceeds through the more stable carbocation intermediate.
d)
The C-H and C-X bonds that break must be anti.
91.
Which statement best describes the reaction?
a)
An E2 with coplanar orientation
b)
An E2 with cis-cis elimination
c)
An E2 that would not occur with this stereochemistry
d)
Neither
92.

Give the name of reaction in the preparation of alkene from alcohol compounds.

a)

Dehydrohalogenation

b)

Hydration

c)

Halogenation

d)

Dehydration

93.

What is the type of reaction in chemical reactions where dehydration occurs?

a)

Addition

b)

Substitution

c)

Rearrangement

d)

Elimination

94.

What type of reaction is shown

a)

Addition

b)

Elimination

c)

Substitution

d)

Replacement

95.
What are elements in groups 3-12 called?
a)
nonmetals
b)
metals
c)
halogens
d)
transition elements
96.

Why is zinc not considered a transition metal?

a)

Zinc is not a transition metal because it gains two 4s electrons to give a 2+ion with full d subshell levels.

b)

Zinc is not a transition metal because it loses four 4s electrons to give a 4+ion with full d subshell levels.

c)

Zinc is not a transition metal because it loses two 4s electrons to give a 2+ion with full d subshell levels.

d)

Zinc is not a transition metal because it gains two 4d electrons to give a 2+ion with full d subshell levels.

97.

The transition elements form a ________ of about 30 Metals in the________ of the Periodic Table.

a)

Block & catalysts

b)

Block & Middle

c)

Catalysts & Coloured

d)

High & Middle

98.
What are the uses of transition elements?
a)
building material
b)
pigment
c)
pigment, building material
d)
cars
99.
Where are transition elements found on the periodic table?
a)
at the top
b)
only at the bottom 
c)
center
d)
center and bottom
100.
Which element is written first in a compound?
a)
transition metal
b)
anion
c)
nonmetal
d)
halogen

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