Each sequential element has one more proton and one electron

(as you go from left to right)

as the nucleus becomes ↑ positive,

all electrons experience a stronger pull toward the center.

"how strong a particular element pulls electrons"

cations: have more protons than electrons, therefore they are strongly attracted to electrons

(aka they really want to get rid of their positive charge).

anions: have more elecs will have a slightly lower effective nuclear charge.

neutral: have an equal # of protons and elecs

(have the lowest eff. nuc charge)

Who has a larger effective nuclear charge(Z_eff):

Na or Mg?

Mg

effective nuclear charge increaes as you go across elements in the same period.

Who will have a bigger prinicipal quantum number H or Fr?

whos electrtons will be held less tightly?

Fr ;

as you go  DOWN a grp prinicipal quantum number increases

its  valence e- will be held less tightly to nucleus

K ;

atomic radii decreases as you go across a period

(recall z_eff increases)

energy required to remove an electron from a gaseous atom or ion

(this requires energy (endothermic))

If the effective nuclear charge is high :

describe the location of the valence e-

the ionization energy

the electron affinity

high z_eff=

valence e- tightly bound to nucleus

HIGH ionization energy

HIGH electron affinity

(aka it takes it alot energy to remove these electrons)

Recall an element doesn't want to have a postive charge it wants to gain e- in order to have a full octet,

so it takes alot more energy to remove the 2nd e-  b/c the element is becoming increasingly positive.

Why do grps 1 & 2 have low electron affinties?

Why do grp 7 have high?

grps 1 & 2 (alkali metals &alkali earth metals) need to lose 1 or 2 e- to achieve their octet.

grp 7 (halogens): only need to gain 1 more e- to achieve their octet so they are the greediest.

electron affinity def

electronegativity def

1.energy released when atom recieves an electron

*(remember if an element is closer to its octet its energy will be lower hence released , that is a very good thing)

2. is a measure of the attractive force that an atom will excert in an electron in a chemical bond, aka its attraction for bonding electrons

metals have a high density

high melting point

For metals in general give high/low for the following:

z_eff (effective nuclear charge)

electronegativity

atomic radius

ionization energy

↓z_eff (effective nuclear charge)

↑electronegativity

↑atomic radius

↓ionization energy

1. For non metals in general give high/low for the following:

   z_eff (effective nuclear charge)

   electronegativity

   electron affinity

   atomic radius

   ionization energy

z_eff (effective nuclear charge)

↑electronegativity,electron affinity

↓atomic radius

↑ionization energy

True or False:

Non metals are good conductors of electricity and heat

+1

(they often lose 1 e- to complete their octet)

+2

(they like to lose 2 electrons in order to complete their 'octet')

"full outer shell"

-1

(prefer to gain 1 e- to complete their octet)

*remember they have 7 electrons

Noble gases:

Why are they stable?

tell high/low:

ionization energy

electronegativites

their valence shell is complete (8e-)

↑ionization energy

almost zero  electronegativites

describe the oxidation states of transition metals

give 2 ex

transition metals have many positive oxidation states

Fe: +1 ,+2

Mn: +2,+3,+6,+7

form many differnt ionic compounds

ex hydration complexes (water)

highly colored solutes and compounds(enchances the low solubility of some compounds) 

Why does P have a lower electron affinity than Si?

(this goes agaist the periodic table trend )

P's electronegativity gives a very stable half filled p oribital

vs

Si only needs 1 more electron to fill its p orbital and therefore is very greedy.

which will have a bigger atomic radius?

anion or cation vs a neutral atom

K- (bigger)

than K

b/c its has gained more e-