Periodic Trends

Question 1

When layers of electrons reduce the pull from the nucleus

Answer 1

shielding effect

Question 2

Noble gases do not

Answer 2

have electronegativity

Question 3

The energy required to remove an electron from the valence shell of an atom

Answer 3

ionization energy

Question 4

The amount of pull on electrons while in a chemical bond

Answer 4

electronegativity

Question 5

The amount of positive pull from the nucleus on electrons

Answer 5

effective nuclear charge

Question 6

Period Trend

Answer 6

any characteristic that changes in a regular position across a row (left to right)

Question 7

Group Trend

Answer 7

any characteristic that changes in a regular pattern down group (top to bottom)

Question 8

Atomic radius left to right

Answer 8

decreasing

Question 9

Atomic Radius top to bottom

Answer 9

increasing

Question 10

Ionization energy left to right

Answer 10

increasing

Question 11

Ionization energy top to bottom

Answer 11

decreasing

Question 12

Electronegativity left to right

Answer 12

increasing

Question 13

Electronegativity top to bottom

Answer 13

decreasing

Question 14

Which group on the periodic table has the lowest ionization energy?

Answer 14

alkali metals

Question 15

Which group on the periodic table has the highest ionization energy?

Answer 15

noble gases

Question 16

atomic radius

Answer 16

size of an atom

Question 17

ionization energy

Answer 17

amount of energy needed to remove an electron from the valence shell of an atom

Question 18

valence electrons

Answer 18

in the highest occupied “n” shell, highest energy s+p electrons

Question 19

electronegativity

Answer 19

amount of pull on an electron an atom has in a chemical bond

Question 20

electron affinity

Answer 20

amount of energy needed to add an electron to the valence shell of an atom

Question 21

what is the atomic radius left to right

Answer 21

the more (+) pull, the smaller the atom gets

Question 22

what is the ionization energy left to right

Answer 22

the more (+) pull makes it harder to remove electrons

Question 23

what is the electronegativity left to right

Answer 23

the more (+) pull creates more pull on the outside of the electron

Question 24

what is the atomic radius top to bottom

Answer 24

more layers make the atom bigger with less pull too

Question 25

what is the ionization energy top to bottom

Answer 25

more layers create less pull making it easier to remove electrons

Question 26

what is the electronegativity top to bottom

Answer 26

more layers reduce the pull on electrons to the nucleus

Question 27

How can we add electrons?

Answer 27

Protons pull electrons into the nucleus, so the more (+) pull there is, the harder it is to remove electrons

Question 28

How can we remove electrons?

Answer 28

The more layers/shields of electrons there are reduce the (+) pull towards the nucleus, making it easier to remove electrons

Question 29

How do we lose electrons while going down the PT?

Answer 29

As you go down, the IE decreases creating a lesser (+) pull of electrons making them to be easily removed

Question 30

How do we gain electrons while going up the PT?

Answer 30

As you go up, the energy levels decrease creating a more (+) pull making it harder to remove electrons

Question 31

The less pull/more layers?

Answer 31

the bigger the atom gets, the easier to remove electrons, and reduces the ability to steal other electrons

Question 32

When nuclear charge increases?

Answer 32

pulls electrons closer making them harder to remove and making the atom smaller.