Atomic Radius/ Ionic Radius/ Electronegativity/ Ionisation Energy/ Solubity

Question 1

What is Atomic Radius?

Answer 1

The distance from the nucleus to the outer most electron

Question 2

Moving Across the Periodic Table Atomic Radius ____________

Answer 2

Moving Across the Periodic Table Atomic Radius DECREASES

Question 3

Why does Atomic Radius DECREASE as you move ACROSS the periodic table?

Answer 3

Atomic Radius decreases as you move across the table as there are more protons and electrons at the same distance, resulting in a stronger attraction, pulling the electrons closer.

Question 4

Moving down the Periodic Table the Atomic Radius_________

Answer 4

Moving down the Periodic Table the Atomic Radius INCREASES

Question 5

Why does Atomic Radius INCREASE as you move DOWN the periodic table?

Answer 5

The outer electron are further away from the nucleus

Question 6

What is Ionic Radius?

Answer 6

The space occupied by an ion in the crystal lattice

Question 7

Positive Ions have a __________ ionic radii than corresponding atomic radii.

Answer 7

Positive Ions have a SMALL ionic radii than corresponding atomic radii.

Question 8

Why do POSITIVE ions have a SMALLER ionic radii than corresponding atomic radii?

Answer 8

The larger positive draws the negative electrons in. Therefore a smaller ionic radius.

Question 9

Negative ions have a __________ ionic radii than corresponding atomic radii.

Answer 9

Negative ions have a LARGER ionic radii than corresponding atomic radii.

Question 10

Why do NEGATIVE ions have a LARGER ionic radii than corresponding atomic radii?

Answer 10

The smaller positive electrons are unable to pull of the negative electrons in; also there is a increase in repulsion between the negative electrons. This results in a overall increase in size.

Question 11

What is Electronegativity?

Answer 11

The power of an atom to attract electrons

Question 12

As you move ACROSS a period the electronegativities ___________________

Answer 12

As you move ACROSS a period the electronegativities INCREASE

Question 13

Why do electronegativities INCREASE as you move ACROSS the periodic table?

Answer 13

There is a stronger attraction because of the stronger nuclear charger, because the have more protons and electrons.

Question 14

As you move DOWN a group the electronegativities ___________________

Answer 14

As you move DOWN a group the electronegativities DECREASE

Question 15

Why do electronegativities DECREASE as you move DOWN the periodic table?

Answer 15

The valence electrons a further away from the nucleus, due to the screening effect caused by the electron orbitals there is a weaker attraction.

Question 16

What is Ionisation Energy?

Answer 16

The amount of energy required to remove one electron from an atom

Question 17

As you move ACROSS a Period there is an _____________ in the first ionisation energy.

Answer 17

As you move ACROSS a Period there is an INCREASE in the first ionisation energy.

Question 18

Why does first ionisation energy INCREASE as you move ACROSS the periodic table?

Answer 18

First Ionisation Energy increase because the nuclear charges on the right side of the table are stronger, making them reluctant to loss electrons.

Question 19

As you move DOWN a Period there is an _____________ in the first ionisation energy.

Answer 19

As you move DOWN a Period there is an DECREASE in the first ionisation energy.

Question 20

Why does first ionisation energy DECREASE as you move DOWN the periodic table?

Answer 20

The is a weaker attraction between the nucleus and its valence electrons, caused by the screening effect of electron orbitals as the distance is greater.

Question 21

Why does ionisation energy increase as you lose more electrons?

Answer 21

Ionisation energy increase because as you lose electrons the positive ion becomes stronger pulling the electrons closer; therefore requiring more energy to remove.

Question 22

Why do atom with Nobel Gas Configurations have highest ionisation energies?

Answer 22

Since they have a full shell they are stable, making them reluctant to lose more; resulting in a higher ionisation energy.

Question 23

What identifies a full shell (ionisation energy)?

Answer 23

The biggest jump in ionisation energy.

Question 24

____________Highest 1st ionisation energy

____________ Lowest 1st Ionisation energy

Answer 24

NOBLE GASES Highest 1st ionisation energy

ALKALI METALS Lowest 1st Ionisation energy

Question 25

SOLUBLE:

Answer 25

NO precipitates form

Question 26

INSOLUBLE:

Answer 26

Precipitate forms