Periodicity and Such

Question 1

What is effective nuclear charge?

Answer 1

The force of attraction of the nucleus on its own electrons, dependent on the screening effect.
Variable: Z(eff)

Question 2

Does atomic radius increase or decrease closer to the bottom and left of the Periodic Table?

Answer 2

It increases.

Question 3

True or false: ionization energy increases toward the top right of the Periodic Table.

Answer 3

True

Question 4

True or false: electron affinity is for removing electrons and ionization energy is for adding them.

Answer 4

False. Electron affinity refers to the addition of an electron to a gas. Ionization energy refers to the removal of an electron from an atom in any state.

Question 5

What is the order of atomic orbitals in terms of lowest to highest energy level?

Answer 5

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d.

Question 6

What is the effect of a high effective nuclear charge on an atom?

Answer 6

The ionization energy will be greater. The atomic size will be smaller.

Question 7

What is the effect of a low effective nuclear charge on an atom?

Answer 7

The ionization energy will be lesser and the atomic size will be greater.

Question 8

Which groups of elements are exceptions to the trend in ionization energies?

Answer 8

Group 3A and group 6A.

Question 9

What is the effect of a high effective nuclear charge on the absorption spectrum of an atom?

Answer 9

Fewer bands of colour will appear, because more energy is needed to excite the electrons.