periodicity: the arrangement of the elements in order of their atomic numbers so that elements with...

Periodicity: The arrangement of the elements in

order of their atomic numbers so that elements with similar properties fall in

the same column, or group.

Atomic Radii-• one-half the distance between the nuclei of

identical atoms that are bonded together.

Trend:

Increasin

g size

Increasing size

Atomic Radii-Why do atoms get smaller as you go from

left to right across a period?periodic trends- atoms get smaller as you go from left to right because of an increasing positive charge of the nucleus more protons (+) = more pull on electrons (-) = smaller atom

group trends- radii get larger down a group because of electrons occupying more energy levels and sublevels more electrons in more energy levels = bigger atom

Why do atoms get larger as you go down a group?

Atomic Radius:

Increasin

g size (m

ore en

ergy levels)

Increasing size (Less protons to pull on electrons)

Which has the greater atomic radius, C or O?

Which has the greater atomic size, Li or K?

Ionization energy-the energy required to remove one

electron from a neutral atom of an element

Trend:

Ionization EnergyWhy does it take more energy to remove an

electron (ionize) as you go from left to right?periodic trends-energy increases across the period because of increasing nuclear charge(as you go left to right, the atomic number increases so the number of protons increases so the charge increases) (more protons = more pull on electrons = harder to remove)

group trends-decrease down the group because electrons are farther away from nucleus. (electrons further from nucleus = less pull on electrons = easier to remove)

Why does it take less energy to remove an electron (ionize) as you go down a group?

Ionization Energy:

Incr

easi

ng

en

erg

y (E

lect

ron

s cl

ose

r to

nu

cleu

s =

h

ard

er t

o r

emo

ve

Increasing energy (More protons = harder to remove electrons)

Which has the higher ionization energy, Mg or P?

Which has the higher ionization energy, As or Sb?

ElectronegativityElectronegativity: a measure of the ability

of an atom in a chemical compound to attract electrons.(does not apply to noble gasses. They don’t form compounds)

Which atom is more electronegative?

Trend:

ElectronegativityWhy do atoms attract electrons more as you

go from left to right?periodic trends- increases across each period because of greater nuclear charge in the atom (does not apply to noble gasses) more protons = more pull on electrons

group trends-decreases or stays the same down a group because electrons are further away from the nucleus. electrons further from nucleus = less pull on electrons

Why do atoms attract electrons less as you go down a group?

Electronegativity:

Incr

easi

ng

(E

lect

ron

s cl

ose

r to

nu

cleu

s =

mo

re

pu

ll o

n e

lect

ron

s)

Increasing (More protons = more pull on electrons)

Which has a higher electronegativity, C or O?

Which has the electronegativity , As or Sb?

Ionic Radii- A cation (a positive ion) formed when a neutral atom

loses electrons

An anion (a negative ion) is formed when an atom gains electrons

Ionic RadiiWhy do atoms get smaller when they lose

electrons?trend- when a neutral atom becomes a cation (+) its radius decreases due to a lower number of electrons in the electron cloudLess electrons = smaller electron cloud = smaller atom

Trend- when a neutral atom becomes an anion (-) its radius increases due to a higher number of electrons in the electron cloud. More electrons = larger electron cloud = larger atom

Why do atoms get larger when they gain electrons?

Increasing: Ionization energy, Electronegativity,

Increasing: Atomic radius (size)

Label your periodic table:

Which atom is more electronegative?

Mg or Sr

Which atom has a higher ionization energy?

Pd or Cd

Which atom has a larger radius?

P or Sb

Which atom has a larger radius?

Ag or Ag2+

Which atom is smaller in size?

Ba or Cr

Which atom requires more energy to ionize?

Sn or Ne