Chemistry Unit 3 - The Periodic Table

Question 1

What group are Alkali Metals a part of?

Answer 1

Group 1

Question 2

What group are Alkaline Earth Metals a part of?

Answer 2

Group 2

Question 3

What groups are Transition Metals a part of?

Answer 3

Group 3-12

Question 4

What group are Halogens a part of?

Answer 4

Group 7A

Question 5

What group are Noble Gases a part of?

Answer 5

Group 8A

Question 6

A highly reactive metal, reacts with water, makes a basic solution with water, conducts electricity

Answer 6

Na (A1 elements)

Question 7

A medium reactive metal, reacts with acid not water, conducts electricity, malleable

Answer 7

Ag (any transition metal)

Question 8

A semiconducting material, solid

Answer 8

Si (any metalloid)

Question 9

A nonreactive gas at room temperature

Answer 9

He (any noble gas)

Question 10

A highly reactive gas at room temperature

Answer 10

F or Cl

Question 11

What is Coulombs Law?

Answer 11

The force (units=newtons) between charged objects is directly proportional to the objects’ charges and inversely squared to the distance between the objects. An attractive force exists within an atom between the positively charged nucleus and the negatively valence electrons.

Question 12

Why does Coulombic Attraction decrease down a group?

Answer 12

Electrons are added to a new PEL, causing the electron cloud to increase in size—> atom size increases
This is an increase in distance between the nucleus and the valence electrons which decreases the force o CA
This causes valence electrons to feel less of a pull —> becomes easier to remove the valence electron

Question 13

Why does Coulombic Attraction increase across a period?

Answer 13

Electrons are added to the ame PEL causing a negligible change in size
Increase in the number of protons in the nucleus causes an increase in total charge which causes an increase in CA
Causes valence electrons to feel more of a pull from the nucleus—> becomes harder to remove valence electrons

Question 14

What is atomic radius?

Answer 14

Measures the size of the atoms from the center of the nucleus to the boundary of the surrounding shells

Question 15

Which element has atoms with the smallest radius?

Answer 15

He

Question 16

Which element has atoms with the largest radius?

Answer 16

Francium

Question 17

Atomic radius trend across a period

Answer 17

<——– (decreases)

Question 18

Atomic radius trend down a group

Answer 18

vvv (increases

Question 19

Atomic radius trend down a group explanation

Answer 19

As you go down a group, CA attraction decreases which mean’s that the nucleus cannot pull valence electrons as much resulting in a larger atomic radius

Question 20

Atomic radius trend across a period explanation

Answer 20

As you go across a period, CA increases meaning that the nucleus can pull in the valence electrons resulting in a smaller atomic radius

Question 21

What is Ionization Energy?

Answer 21

The minimum amount of energy required to remove the most loosely bound electron of a neutral atom

Question 22

Which group has the highest values for ionization energy?

Answer 22

Noble gases

Question 23

Which group has the lowest values for ionization energy?

Answer 23

Alkali metals

Question 24

IE trend across a period

Answer 24

—–> (increases)

Question 25

IE trend down a group

Answer 25

^^^ (decreases)

Question 26

Why does IE decrease down the group?

Answer 26

As CA decreases down a group, nucleus’ attractive power decreases which causes less pull on the valence electrons. With less pull, electrons require less energy to remove and are thus easier to remove resulting in a lower IE

Question 27

Why does IE increase across the period?

Answer 27

As CA increases across the period, nucleus’ attractive power increases which causes more pull on the valence electrons. With more pull, the electrons require more energy to remove and are thus harder to remove resulting in a higher IE

Question 28

What is electronegativity?

Answer 28

Measures the tendency of an atom to attract a shared pair of electrons toward itself

Question 29

Which element is the most electronegative?

Answer 29

Fluorine

Question 30

Which element is the least electronegative but not zero?

Answer 30

Francium

Question 31

Trend of electronegativity across a period

Answer 31

—–> (increases)

Question 32

Trend of electronegativity down a group

Answer 32

^^^ (decreases)

Question 33

Why does EN decrease down a group?

Answer 33

As CA decreases down a group, the nucleus’ attractive power decreases which causes less pull on the valence electrons. With less pull, electrons aren’t attracted easily which is why EN also decreases

Question 34

Why does EN increase across the period?

Answer 34

As the CA increases across the period, the nucleus’ attractive power increases which causes more pull on the valence electrons. WIth more pull, electrons are attracted more easily causing an increase in EN