periodic table

Question 1

elements in a group has similar chemical properties

Answer 1

why: same number of valence electrons

Question 2

atomic radius - down a group

Answer 2

distance between the nucleus and the furthest electron
- increases as you go down
- why: more occupied pels (rings), creates a greater distance between the nucleus and its furthest electron

Question 3

ionization energy (IE) - down a group

Answer 3

the amt of energy needed to remove the most loosely bound electron from its valence shell
- decreases as you go down a group
- why: atoms with a larger radius has valence electrons that are further away from the nucleus, making easier to lose electrons

Question 4

electronegativity (EN) - down a group

Answer 4

a measure of attraction of a nucleus of one atom for another atom’s valence electrons
- decreases as you go down a group
- atoms with a big radius have low EN. attraction for another atom’s electrons decreases with more occupied rings because its nucleus is further from another atom’s valence shell

Question 5

metallic property - down a group

Answer 5

measure of how easily an element loses electrons
- the metallic properties increases as you go down the group; lose electrons easily
- elements on the bottom of the group have LOW EN and LOW IE, so they lose electrons very easily / react very easily

Question 6

atomic radius - across a period

Answer 6

decreases across a period
- greater nuclear charge
- more protons pull the electrons closer to the nucleus and the radius increases

Question 7

ionization energy - across a period

Answer 7

increases across a period
- takes more energy to remove electrons from non-metals than metals
- why: greater nuclear charge; electrons are held closer to the nucleus due to a smaller radius

Question 8

electronegativity - across a period

Answer 8

increases across a period
- more attraction for another atom’s electrons
- why: greater nuclear charge; distance between that atom’s and another atom’s electrons decreases