Periodic Trends 5

Question 1

As you _ atomic radius decreases

Answer 1

Move across a period from left to right

Question 2

Why atomic radius decreases when you move from left to right of a period

Answer 2

The effective nuclear charge increases as electrons are added to the energy level

Question 3

As electrons are added to the energy level which is

Answer 3

The same distance from the nucleus

Question 4

Atomic radius increases from top to bottom in a group as

Answer 4

The effective nuclear charge decreases

Question 5

Effective nuclear charge decreases due to

Answer 5

More electrons in more energy levels

Question 6

Magnesium has a larger atomic radius (is bigger) than

Answer 6

Chlorine

Question 7

Magnesium is bigger than chlorine because

Answer 7

It is to the left on periodic table

Question 8

Magnesium has 12 protons and _ neutrons

Answer 8

12

Question 9

Chlorine has 17 protons and _ neutrons

Answer 9

18

Question 10

Ionic radius is the distance between the center of

Answer 10

The nuclei of two ions that barely touch

Question 11

Ionic radius increases for

Answer 11

Nonmetals moving across a period

Question 12

Effective nuclear charge definition

Answer 12

Force of attraction exerted by the protons

Question 13

Ionic radius increases for nonmetals moving across a period because

Answer 13

Effective nuclear charge decreases as number of electrons exceeds number of protons

Question 14

For a neutral atom _ are equal (2)

Answer 14

Atomic radius

Ionic radius

Question 15

Ionic radius increases as

Answer 15

Ion gains electrons

Question 16

In atoms that have a charge _ are unequal

Answer 16

Atomic radius

Ionic radius

Question 17

Ionic radius _ for metals moving left to right across a period

Answer 17

Decreases

Question 18

Reason why metal’s ionic radius decreases from left to right

Answer 18

Because they lose elections (effective nuclear charge increases)

Question 19

The greater the nuclear charge, the more power being used to

Answer 19

Pull the electrons more tightly together

Question 20

IE stands for

Answer 20

Ionization energy

Question 21

Ionization energy is the energy required to remove one or more electron from _

Answer 21

A neutral atom in the gas phase

Question 22

Not all atoms can _

Answer 22

Give up electrons easily

Question 23

In materials that hold electrons loosely the _ is relatively easy to pull off

Answer 23

Electron that is farthest from the nucleus

Question 24

IE decreases from _ to _ in a group

Answer 24

Top

Bottom

Question 25

As you move down a group, size increases as

Answer 25

Electrons are added in energy levels farther from the nucleus

Question 26

The bigger the atoms, the less

Answer 26

Ionization energy is needed to pull the electrons off

Question 27

Farther away electrons are from nucleus, (bigger atom)

Answer 27

The weaker the attraction of the nucleus

Question 28

IE increases going from _ to _ across the periodic table

Answer 28

Left

Right

Question 29

As you move across a period, the effective nuclear charge increases as ()

Answer 29

Electrons are added at the same distance from the nucleus (making it harder to remove electrons)