Chapter 6 (HARD)

Question 0

Describe how the periodic table developed overtime.

Answer 0

1829- Dobereiner Triads (organized by chemical properties)
1864- Newlands Law of Octaves (every 8 elements have similar
properties) Organized left to right by increasing atomic mass
1869- Mendeleev (arranged by increasing atomic mass and
properties)
Today- rows (arranged by atomic number)
Columbus (arranged by similar properties)

Question 1

Define periodic law and what it means to be periodic

Answer 1

Periodic law- the elements are arranged in increasing atomic number.

Periodic- something that happens every once and a wile

Question 2

Compare and contrast metals, nonmetals, and metalloids

Answer 2

Metals- most elements (80%)
Good conductors of heat
Shiny (high luster)
Solid at room temp.

Nonmetals- upper right of the periodic table
Gasses at room temperature
Poor conductors of heat and electricity

Metalloids- general qualities of metals and nonmetals
Controlled by changing conditions. Semiconductors

Question 3

Memorize the names and locations of groups on the periodic table

Answer 3

Group 1- Alkali Metals
Extremly reactive
Explosive reaction in water

Group 2- Alkali Earth Metals
Reactive and has 2 valence electrons

Group 3-16
They all metals

Group 17- Halogens
Nonmetals and 7 valence electrons
Combined with metals= make salts

Group 18- Noble Gases
Gases at room temp.

Question 4

Define group/family and period

Answer 4

Group/ family= a column (18 of them)

Period= a row

Question 5

Compare and contrast:

Different groups
Names
Location/ group number
Reactivity 
Electron Configuration
Number of valence electrons

Answer 5

See 6-1 notes (yellow tab thing)

Question 6

Diagram how an atomic radius is measured

Answer 6

Two atoms are next to each other. 1/2 the distance between the two nuclei

Question 7

Describe how ions form

Answer 7

When electrons are transferred between atoms.

Question 8

Is an ion smaller or larger then the atom size

Answer 8

Cation - Smaller size 
              Positive charge (loses -e)

Anion- Larger size
            Negative charge (adds -e)

Question 9

Define three periodic trends as well as explain what causes the trends

Answer 9

Atom size (largest= bottom left)
       The greatest amount of electron shielding (pushes stuff apart)
Ionization energy (largest= top right)
       Greater nuclear charge, more pull= harder to remove outer 1
Electronegativity (largest= top right)
       The nuclear charge increases= greater pull. Fluorine= most

Question 10

Define electron shielding and nuclear charge

Answer 10

Electron shielding- the inner, lower energy electrons that block the
pull of the nucleus on the outer electrons
Nuclear charge- always a positive charge

Question 11

Ionization energy

Answer 11

Ionization energy- the amount of energy required to remove to
remove the outer electron