Periodicity

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8 questions

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Which of the following factors generally decrease in size as you move from left to right across a period on the periodic table?

Both atomic radius and ionization energy

Atomic radius

Successive ionization energies

Ionization energy

Which type of ion typically has a larger radius than its parent atom?

Transition ions

Valence ions

Anions

Cations

Why does ionization energy generally increase as you move from left to right across the periodic table?

Because atomic radius increases

Because increasing effective nuclear charge pulls electrons in more tightly

Because electron shielding decreases

Because of decreasing effective nuclear charge

What is the trend in successive ionization energies for an atom?

They remain constant after the first ionization

They decrease with each successive ionization

They increase with each successive ionization

There is no general trend in successive ionization energies

The successive ionization energies for element X are given below: IE1=250 kJ mol−1 IE2=820 kJ mol−1 IE3=1100 kJ mol−1 IE4=1400 kJ mol−1 Find out the number of valence electrons from the element X.

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3

4

Which group of elements in the periodic table has the highest electronegativity?

Halogens (Group 17)

Alkali Metals (Group 1)

Transition metals (Groups 3-12)

Noble Gases (Group 18)

Which list describes an arrangement of elements from group II of the periodic table in the order of increasing ionisation energy?

Ba, Sr, Ca, Mg, Be

Be, Mg, Ca, Sr, Ba

Sr, Ba, Ca, Mg, Be

Ba, Be, Ca, Sr, Mg

Which of the following equations correctly represents the second ionisation energy of the element sodium?

Na + I.E.→Na++e -

Na+ + I.E.→Na2++e-

Na + I.E.→Na+2+e−

Na2+ + I.E.→Na3++e−

Which of the following factors generally decrease in size as you move from left to right across a period on the periodic table?

Both atomic radius and ionization energy

Atomic radius

Successive ionization energies

Ionization energy

Which type of ion typically has a larger radius than its parent atom?

Transition ions

Valence ions

Anions

Cations

Why does ionization energy generally increase as you move from left to right across the periodic table?

Because atomic radius increases

Because increasing effective nuclear charge pulls electrons in more tightly

Because electron shielding decreases

Because of decreasing effective nuclear charge

What is the trend in successive ionization energies for an atom?

They remain constant after the first ionization

They decrease with each successive ionization

They increase with each successive ionization

There is no general trend in successive ionization energies

The successive ionization energies for element X are given below:
IE1=250 kJ mol−1
IE2=820 kJ mol−1
IE3=1100 kJ mol−1
IE4=1400 kJ mol−1
Find out the number of valence electrons from the element X.

1

2

3

4

Which group of elements in the periodic table has the highest electronegativity?

Halogens (Group 17)

Alkali Metals (Group 1)

Transition metals (Groups 3-12)

Noble Gases (Group 18)

Which list describes an arrangement of elements from group II of the periodic table in the order of increasing ionisation energy?

Ba, Sr, Ca, Mg, Be

Be, Mg, Ca, Sr, Ba

Sr, Ba, Ca, Mg, Be

Ba, Be, Ca, Sr, Mg

Which of the following equations correctly represents the second ionisation energy of the element sodium?

Na + I.E.→Na++e -

Na+ + I.E.→Na2++e-

Na + I.E.→Na+2+e−

Na2+ + I.E.→Na3++e−