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Chemistry Chapter 3
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period
elements in the same horizontal row
same number of energy shells
group
elements in the same vertical column
same number of valence electrons
Group IA (1A)
alkali metals
1 valence electron
Group IIA (2A)
alkali earth metals
2 valence electrons
Group VIIA (7A)
halogens
7 valence electrons
Group VIIIA (8A)
noble gases
8 valence electrons
Transition Metals
Group 3-12
shell
location and energy of electrons around a nucleus (n)
> n = > energies/distances
subshell
each shell made up of one or more subshells
s, p, d, f
number of subshells = number of the shell (shell 3 contains 3s, 3p, 3d)
identify shell by shell #, subshell letter (3p subshell)
orbital
specific volumes of space around the nucleus where electrons move
s subshell - 1 orbital - 2 electrons
p subshell - 3 orbitals - 6 electrons
d subshell - 5 orbitals - 10 electrons
f subshell - 7 orbitals - 14 electrons
Two electrons per orbital
Subshell Filling
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d
Electron Configurations
Gallium 31 electrons 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
4p
1
Noble Gas Configurations
Electronic configurations of noble gases end with completely filled s and p subshells
He
: 1s
2
Ne
: [He]2s
2
2p
6
Ar
: [Ne]3s
2
3p
6
Kr
: [Ar]4s
2
4p
6
Xe
: [Kr]5s
2
5p
6
Example: Mg -> [Ne]3s
2
Metallic Property Trends
elements become less metallic left to right across periods
elements become more metallic top to bottom down group
Atom Size Trends
elements become smaller left to right across periods
elements become larger top to bottom down group
ion
atom or molecule where electrons do not equal protons (net positive or negative charge)
cation
positive
charge
has lost electrons
metals
anion
negative charge
has gained electrons
nonmetals
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Author
tiffanydawnn
ID
24032
Card Set
Chemistry Chapter 3
Description
Electronic Structure/Periodic Law
Updated
2010-06-18T17:13:55Z
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