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Flashcards in Chapter 6 (HARD) Deck (12):

Define periodic law and what it means to be periodic

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

Periodic- something that happens every once and a wile


Describe how the periodic table developed overtime.

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
Today- rows (arranged by atomic number)
Columbus (arranged by similar properties)


Compare and contrast metals, nonmetals, and metalloids

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


Memorize the names and locations of groups on the periodic table

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.


Define group/family and period

Group/ family= a column (18 of them)
Period= a row


Compare and contrast:

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

See 6-1 notes (yellow tab thing)


Diagram how an atomic radius is measured

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


Describe how ions form

When electrons are transferred between atoms.


Is an ion smaller or larger then the atom size

Cation - Smaller size
Positive charge (loses -e)

Anion- Larger size
Negative charge (adds -e)


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

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


Define electron shielding and nuclear charge

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


Ionization energy

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