Atoms tend to gain, lose, or share electrons until they are surrounded by eight valence elctrrons.

consist of full s and p subshells

Indicates how easily an electron can be removed from an atom.

first ionization energy is the energy needed to remove the first electron. the second ionization energy is the energy needed to removed the second electron...etc.

the GREATER the ionization energy, the more difficult it is to remove an electron because the more energized electrons are pulling towards the nucelus.

measures how easily an atom can gain an electron.

The lattice energy of an ionic solid is a measure of the strength of bonds in that ionic compound.

- the L energy increases as the charge increases.

- the L energy increases as their ionic size decreases.

TO ORGANIZE IONS IN INCREASING OR DECREASING L. ENERGY:

1.first determine the charges on their ions (refer to the back of the book).

2. if some of the ions are equal, arrange them in ionic size.  the smaller the ion, the more L. energy is has.

the number of valance elctrons in a nuetral atom is the same as the group number.

must fulfill octect rule

draw valance elctrons first

then draw bonds

each atom must have 8 e- (other than H)

Arranged elements in order of increasing atomic weight.

-Forerunner of the periodic table.

- Given credit for predicting Ga and Ge.

Lothar Meyer did the same thing in Germeny.

developed the concept of atomic numbers.

- he found the each element produces a frequency and that frequncey increases as the atomic mass increases.

- he correcrtly identified that the atomic number is the same as the number of protons in the atom.

he distance separating the nucleii of two atoms in a molecule.

-the bonding atomic radius is shorter than the nonbonding atomic radius.

the bonding atomic radii is 1/2 of the bonding distance.

radius INCREASES going down a column.

(because the outter elctrons are farther from the nucleus, giving the atoms a larger size)

radius INCREASES going right of a row.

(because the increasing effective nuclear charge draws the electrons closer to the nucleus, giving the atoms a smaller size.)

smaller - because of the loss of elctrons decreases their atomic radii.

a groups of ions all having the same number of elctrons.

TO ARRANGE THESE IONS: place the ions in order of increasing atomic number.

In a ROW,  the energy increases with increasing atomic number (moving right).

In a COLUMN, the energy decreases with increasing atomic number (moving down)

effective nuclear charge

and

average distance of the electron from the nucleus.

solid

(except mercury)

OXIDIZED

(lose electrons)

1. low densities

2. low metling points

3. lowest ionization energy

4. very reactive to lose an electron to form a cation

5. exsist in nature as compounds only.

6. these metals directly combine with nonmetals.

7. act vigorously with water to produce hydrogen gas and hydroxide solution.

8.when O reacts with these metals, O2- is formed.

9. metal oxides react with water to form hydroxide ions

10. emits a characteristic color when placed in a flame.

Hydride.

(When hydrogen gains an electron)

1. solid at room temp

2. less reactive than group 1A

3. Be and Mg ar ethe lightest and less reactive.

4. tend to lose outter shell electrons and form 2+ cations.

5. the heavier the metals give off  colors when under a flame.

6. fireworks: emit colors from group 2A elements.

1. does not lose it's valence electron easily.

2. shares it's electron with nonmetals and forms molecular compounds

3. able to form covalent bonds

4. able to form metal hydroxides

5. able to lose an electron to form a 1+ cation (H+)

1. colorless at room temp

2. O3: ozone

3.great tendency to attract electrons

4. sulfur has a tendendy to gain electrons also.

1. salt formers

2. nonmetals

3. melting and boiling points increase with increasing atomic number

4. diatomic molecules

5. highly negative electron affinities

6. tend to gain electrons to form halide ions

7. Cl is the most useful halogen

8. all soluble in water

1. all nonmetals, gas at room temp

2. monatomic

3. largest ionization energy

4. unreactive