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PERIODIC TABLE 2M1S10

Total questions: 25

Worksheet time: 29mins

Name
Class
Date
1.

The electronic configuration of M is 1s2 2s2 2p6 3s2 3p6 4s2 3d1. Determine the group and period.

a)

Group 2 Period 4

b)

Group 3 Period 4

c)

Group 3 Period 3

d)

Group 13 Period 3

2.

Arrange the following atoms in an ascending order of their radii.

P , Si, Al, Cl, Ar,S

a)

Al<Si<P<S<Cl<Ar

b)

Al>Si>P>S>Cl>Ar

c)

Al>Si>P>S>Cl>Ar

d)

Ar<Cl<S<P<Si<Al

3.

In which one of the following sequences are the oxides of the elements classified as basic, amphoteric and acidic?

a)

Mg, S, Al

b)

Na, K, S

c)

Na, Mg, Al

d)

K, Al, P

4.

Cations are smaller than their corresponding atoms. Why?

a)

The atom removes an electron to form cation.

b)

The electron cloud repels each other

c)

The mutual repulsion stronger

d)

The effective nuclear charge of cation higher

5.

Which of the equation below refers to the electronegativity?

a)

O (g) + e  →\rightarrow  O+(g)

b)

O (g) + e  \rightarrow  O-(g)

c)

O(g) + e  \rightarrow  O2-(g)

d)

O (g) + 2e  \rightarrow  O2(g)

6.

Which is the most electronegative element in Group 15?

a)

N

b)

Cl

c)

F

d)

O

7.

Which of the following series of atoms show the correct order of decreasing first ionisation energy?

a)

Na>Li>H

b)

Be>Mg>Ca

c)

C>N>O

d)

Cl<S<P

8.

Which of the following can form isoelectronic series?

a)

N, O, Ne, Mg

b)

B, Al, Ga, In

c)

Cl, Br, Ar, Kr

d)

Li, Be, Na, Mg

9.
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
10.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
11.
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
12.

Which of the following elements has the smallest atomic radius?

a)

Sulfur

b)

Chlorine

c)

Aluminum

d)

Sodium

13.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

14.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

15.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium (He)

b)

Titanium (Ti)

c)

Calcium (Ca)

d)

Magnesium (Mg)

16.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
17.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

18.

As you look from left to right across a period, electronegativity

a)

increases

b)

decreases

19.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
20.

Who developed the Periodic Table?

a)

Mendeleev, who was a chemist and teacher

b)

Pavlov, who was a teacher and physchologist

c)

Ladahoff, who was a teacher and biologist

21.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
22.

The electronegativity of Cl is the highest in Period 3. Why?

a)

Cl is the largest and has the greatest effective nuclear charge

b)

Cl is the smallest and has the lowest effective nuclear charge

c)

Cl is the largest and has the lowest effective nuclear charge

d)

Cl is the smallest and has the greatest effective nuclear charge

23.
The energies of electrons as they orbit the nucleus of an atom
a)
energy levels
b)
orbits
c)
shells
d)
electron area
24.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
25.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration

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