Chemistry Flashcards
(34 cards)
atomic mass vs atomic weight
mass is roughly protons + neutrons
weight is the average mass of isotopes (on periodic table)
both in amu units
quantum numbers
n, l, ml, ms
describes position + energy of electron in an atom (energy states)
n quantum number
- number of shells
- max # of e in a shell = 2n^2
l, azimuthal quantum number
- refers to shape and number of subshells
-possibility of subshells = (n - 1)
(n=3 can have subshell 0, 1, 2)
-max number of e in a subshell = 4l + 2
-s, p, d, f, = examples of subshells
ml magnetic quantum number
- refers to the orbital of a subshell
- number of orbitals in a subshell = -l to +l, including 0 (ex. l=1 ml= -1,0,+1)
ms spin quantum number
- electrons can spin up or down (half arrows)
- -(1/2) or + (1/2)
electron configuration
(read periodic table)
-spdf
hunds rule electron configuration
draw out elec. config
in order with electrons starting in lowest to highest orbital
-number of spots = ml of orbital
Exceptions to the electron configuration rule
Chromium (Z=24) [Ar] 4s^1d^5
Copper (Z= 29) [Ar] 4s^1 3d^10
Metals
middle to left of the periodic table (not Hydrogen), including lanthanides + actinides
(opposite of non-metals)
-easily give up e-, good conductors or heat and E
-low effective nuclear charge
-low electroneg, high electropositivity
-large atomic radius, low ionization energy
-malleable
Non-metals
upper right of periodic table
- high electronegativity + ionization E
- small atomic radii
- don’t give up e easily
- poor conductors
- brittle solids
Metalloids
stair step group btw metal + nonmetals
-the in between of metals + non-metals
effective nuclear charge (Zeff) + periodic table trend
pull of e- to nucleus
-for the most part more e- in valence = more pull (Zeff)
(left to right increasing)
compare directly up and down, up is stronger
Atomic radii + periodic table trend
- half the distance between 2 atoms in contact
- decreases left to right (Zeff pulls valence e- in)
- radius increases going down
ionic radii + periodic table trend
- nonmetals: gain e- and become more negative
- nonmetals closer to metalloids line have larger ionic radii
- metals: lose e- and become more positive
- metals closer to metalloids are smaller
Ionization Energy + periodic trends
- endothermic (requires energy) to removing an e- -greater Zeff, harder to remove e-, increasing ionization E -Increases to right, decreasing down
- increases w/ each ionization
electron affinity
- exothermic, gain an e-
- increasing to the right (to complete the octet)
- decreases going down
electronegativity
-highest towards F (similar to ionization energy)
_exclude noble gases
alkali metals
- +1 charge typically (only 1 valence e-)
alkaline earth metals
- +2 charge typically
halogens
- 7 valence e-, highly reactive
- often form bond with itself (gas)
exceptions to the octet rule
incomplete octet - lass than 8 (H (2), He (2), Be (4), B(6)
expanded - more than 8 (period higher than 3/d orbital)
P(10), S (12), Cl (14)
odd number of e- can’t distribute an e- to give 8 (NO, had 11 e-)
Coordinate covalent bond
Lewis acid/base
Type of reactions
- Neuralization: type of DD rxn acid + base form a salt and h20
- combination
- decomposition
- combustion: fuel** hydrocarbon + oxidant (typically 02) to get H2O + CO2
- Single displacement: usually a redox
- double displacement: swapping (1 metal +nonmetals)
