Free Printable SK015- 3.2 Periodicity- Part B

Worksheets

SK015- 3.2 Periodicity- Part B

Total questions: 15

Worksheet time: 8mins

Name

Class

Date

Ionisation energy is ___________.

maximum energy required to remove 1 electron from 1 mol of gaseous atom

minimum energy required to remove 1 electron from 1 mol of gaseous atom

first ionisation energy

second ionisation energy

When across a period, the atomic size decreases so the first IE ___________.

increases

decreases

constant

i am not sure

When going down a group, the atomic size increases so the first IE __________.

increases

decreases

constant

I am not sure

Factors affecting the ionisation energy:

Atomic radius

Effective nuclear charge

Shielding effect

All of the above

The equation for the first ionisation energy of a sodium atom is:

Na (g) -> Na⁺ (g) + e^-

Na⁺ (g) -> Na²⁺ (g) + e^-

Na (s) -> Na⁺ (g) + e^-

Na⁺ (g) + e^- -> Na (g)

Which has the lower first ionisation energy between magnesium and aluminium elements and why

Magnesium because it has a lower nuclear charge and higher atomic radius

Aluminium because it has fewer protons

Magnesium because its outermost electron is removed from an orbital further from the nucleus

Aluminium because it is removed from an orbital which is higher in energy

Why is the fifth ionisation energy IE₅of carbon is so much larger than the fourth ionisation energy IE₄?

Tips: Write out electronic configuration

due to removal of electron from the stable half- filled 2p orbital

due to removal of electron from the stable fully- filled 2p orbital

due to removal of 5th electron from the inner 2s orbital

due to removal of 5th electron from the inner 1s orbital

Element G has nucleon number 24 and proton number 12. Select the type of oxide formed by element G and the formula of oxide.

basic

acidic

amphoteric

GO₂

From which one of the following particles is it most difficult to remove an electron?

Cl^- (g)

Ca⁺(g)

Na⁺(g)

Ar(g)

10.

An element X has the following successive ionisation energies, in kJ mol^-1?

578 (1st), 1817, 2745, 11575, 14830, 18376, 23293

Which one of the following is possibly element X?

11.

The first seven ionisation energies of an element in Period 2 in the Periodic Table are as follows.

1310, 3390, 5320, 7450, 11 000, 13 300, 71 000

What is the outer electronic configuration of the element?

2s²

2s²2p¹

2s²2p⁴

2s²2p⁶

12.

A simple ion X⁺ contains eight protons. What is the electronic configuration of X⁺?

1s² 2s¹2p⁶

1s² 2s²2p³

1s² 2s²2p⁵

1s² 2s²2p⁷

13.

The correct order of sub-shell notation is:

1s, 2s, 2p, 2d, 3s, 3p, 4s, 3d, 4p

1s, 2s, 2p, 2d, 3s, 3p, 3d, 4s, 4p

1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p

14.

Which equation gives the definition of the first ionisation energy of bromine?

Br(g) --> Br^-(g) - e−

Br(g) --> Br⁺(g) + e−

1/2Br₂(g) --> Br^-(g) - e−

1/2Br₂(g) --> Br⁺(g) + e−

15.

Which element in the Periodic table has the electron configuration 1s²2s²2p⁶3s²3p⁶3d³4s²

a Group 2 element

a Group 15 element

a Group 13 element

a transition metal

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SK015- 3.2 Periodicity- Part B

Total questions: 15

Worksheet time: 8mins

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