Types of elements/periodic properties

Question 1

metals - atomic properties

Answer 1

left side of periodic table
low effective nuclear charge - electrons not strongly held by nucleus
low electronegativity
low ionization energy
large radius

Question 2

nonmetals - atomic properties

Answer 2

smaller group in the upper right hand corner
high effective nuclear charge - more protons, attract electrons and pull their own electrons toward the nucleus
high electronegativity
high ionization energy
small radius

Question 3

Metalloids

Answer 3

stair-step group between metals and non-metals

intermediate properties

Question 4

metals - physical properties

Answer 4

soft, shiny at STP
malleable
ductile - can be drawn into thin wire

Question 5

non-metals - physical properties

Answer 5

any phase at STP
brittle when solid
poor conductors
non-ductile

Question 6

What is effective nuclear charge?

Answer 6

Zeff = # protons - #nonvalence e- (attraction from nucleus-replusion from valence e)
Level of attractiveness between the positively charged nucleus and the negatively charged valence electrons
valence electrons are repelled by non valence (inner shell) electrons, decreasing ENC

Question 7

What is the periodic trend of effective nuclear charge?

Answer 7

increases from left to right
b/c #protons increases from left to right, but # non-valence electrons stays the same
increases from bottom to top due to decreasing distance from nucleus to valence shell (more shells as you go down a group)

Question 8

atomic radius

Answer 8

distance between center of nucleus and outermost electron shell
increasing Zeff = decreasing atomic radius
increases from right to left, top to bottom

Question 9

ionic radii

Answer 9

anions - larger radii due to increased valence electrons
cations - smaller radii due to decreased valence electrons
atomic radii decreases as ion becomes more positive

Question 10

ionization energy

Answer 10

energy required to remove and electron
increases from left to right, bottom to top
gaps between 1st/2nd/3rd IE are greater when it causes the atom to move from a stable state

Question 11

electron affinity

Answer 11

energy released when an electron is gained by an atom in gaseous state
highest in halogens - adding one e makes them noble gases

Question 12

electronegativity

Answer 12

ability of an atom to pull/hog electrons in a bond
greatest for atoms with high effective nuclear charge
increases from left to right, bottom to top
FON