Flashcards in Chapter 6 (HARD) Deck (12):
0
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
1
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
properties)
Today- rows (arranged by atomic number)
Columbus (arranged by similar properties)
2
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
3
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.
4
Define group/family and period
Group/ family= a column (18 of them)
Period= a row
5
Compare and contrast:
Different groups
Names
Location/ group number
Reactivity
Electron Configuration
Number of valence electrons
See 6-1 notes (yellow tab thing)
6
Diagram how an atomic radius is measured
Two atoms are next to each other. 1/2 the distance between the two nuclei
7
Describe how ions form
When electrons are transferred between atoms.
8
Is an ion smaller or larger then the atom size
Cation - Smaller size
Positive charge (loses -e)
Anion- Larger size
Negative charge (adds -e)
9
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
10
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
11