Periodic Trends

Question 1

What scientist is credited for creating the periodic table?

Answer 1

• Demitri Mendeleev
• Published his version in 1869
• Periodic Law

Question 2

There are _ vertical columns in the Periodic Table which are called _

Answer 2

• 18
• Groups

Question 3

There are _ horizontal rows in the Periodic Table which are called _

Answer 3

• 7
• Periods

Question 4

The majority of elements in the Periodic Table are _ which are mostly located on the _ side of the table

Answer 4

• Metals
• Left

Question 5

The minority of elements in the Periodic Table are _ which are mostly located on the _ side of the table

Answer 5

• Nonmetals
• Right

Question 6

There are 6 elements in the _ that are located in the boundary of metals and non-metals.

Answer 6

• Metalloids

Question 7

How are the elements aranged on the periodic table?

Answer 7

They are arranged based on their similarities in electron configuration and they are grouped by their valence electrons.
(‘s’ block, ‘p’ block, ‘d’ block, ‘f’ block)

Question 8

Which two groups of elements are in the ‘s’ block?

Answer 8

Alkali Metals and Alkaline Earth Metals

Question 9

Group 1

Answer 9

• Alkali Metals
• 1 ve
• Lose 1
• Very Reactive

Question 10

Group 2

Answer 10

• Alkaline Earth Metals
• 2ve
• Lose 2e
• Reactive

Question 11

Groups 3-12

Answer 11

• Transition Metals
• Various # of ve
• Low Reactivity (Ex/ will react w/ oxygen in the air but slowly)

Question 12

Group 16

Answer 12

• Oxygen Group
• 6ve
• Gain 2ve
• Reactive (like its counterpart in group 2)

Question 13

Group 17

Answer 13

• Halogen (Means “Self-forming”)
• 7ve
• Gain 1ve
• Very Reactive (Nonmetal- Very reactive like counterpart in Group 1)

Question 14

Group 18

Answer 14

• Nobel Gass
• 8ve
• Gain/Lose None
• Nearly Inert (means not generally reactive)

Question 15

Octet Rule

Answer 15

Atoms with either gain or lose electrons to have a full outer shell of 8ve
Full Shell = Stability

Question 16

Colombic Attraction Force

Answer 16

F = kq1q2/d2

k: Columbs constant
q1: Charge in first particle
q2: Charge in second particle
d: Distance between the two charged particles

Question 17

The higher the _ the stonger the __

Answer 17

1. Charge (# of protons)
2. Attractive Force

Question 18

The longer the _ the weaker the __

Answer 18

1. Distance (from the nucleus to the ve)
2. Attractive Force

Question 19

Atomic Radius

Answer 19

1. The average distance between the nucleus and the ve
2. Usually measured as one-half distance between two nuclei of an element in its elemental form

Question 20

Electronegativity

Answer 20

A measure of the ability of an atom to attract other electrons when the atom is part of a compound

Question 21

Ionization Energy

Answer 21

The energy required to remove 1 electron from an atom

Question 22

The # of _ is dominant
It _ across a period
Attractive Force _ from across a period

For elements in the same period

Answer 22

1. Protons
2. Increases
3. Increases

Question 23

Atomic Radius _ across a period

For elements in the same period

Answer 23

Decreases

Deaceases when there are less protons

Question 24

Electronegativity _ across a period

For elements in the same period

Answer 24

Increases

Question 25

Ionization Energy _ across a period | For elements in the same period

Answer 25

Increases

Question 26

The _ between the nucleus and ve is dominant It _ down a group Attractive Force _ down a group | For elements in the same group

Answer 26

1. Distance 2. Increases 3. Decreases

Question 27

Atomic Radius _ down a group | For elements in the same group

Answer 27

increases | It increases bc/ there are more shells

Question 28

Electronegativity _ down a group | For elements in the same group

Answer 28

Decreases

Question 29

Ionization Energy _ down a group | For elements in the same group

Answer 29

Decreases

Question 30

Electronegativity _ from left to right within a period and _ from top to bottom within a group

Answer 30

1. Decreases 2. Increases

Question 31

As you move down a group, why does atomic radius increase?

Answer 31

It increases because there are more shells (energy levels)

Question 32

Which has greater electronegativity: N or C?

Answer 32

N

Question 33

What element has the lowest ionization energy in group 1 and why?

Answer 33

Cesium (Cs) It is the lowest bc/ itd 1 ve is very far from the nucleus, so very little energy is needed to remove it

Question 33

What element has the lowest ionization energy in group 1 and why?

Answer 33

Cesium (Cs) It is the lowest bc/ itd 1 ve is very far from the nucleus, so very little energy is needed to remove it

Question 34

What atom has the largest atomic radius in period 4?

Answer 34

K

Question 35

The energy required to remove electrons

Answer 35

Ionization Energy

Question 36

What element has the smallest ionization energy in period 5?

Answer 36

Rb

Question 37

As you move across the periodic table, why do atoms tend to get smaller?

Answer 37

Because the atoms have more protons

Question 38

The ability of an atom to attract other electrons

Answer 38

Electronegativity

Question 39

What atom has the largets atomic radius in group 18?

Answer 39

Rn

Question 40

As you move across the periodic table from left to right, the atomic radius . Why?

Answer 40

1. Decreases 2. This is bc/ the number of protons increses, so attraction to electrons increases

Question 41

Elements in the same group will all have similar _

Answer 41

Properties

Question 42

Group 3-12 is known as the _

Answer 42

Transition Metals