Chem 111- Test 3- St. Thomas Flashcards by Alessia Velasquez Nitti

absorbance

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emission

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orbital diagram

the thing w the lines

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electron configuration

[the last nobel gas in row 18] and then the d, s, and p’s

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what doesn’t need 8 around central atom

B and Be

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principle quantum number

n. the shells

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angular momentum or azimuthal quantum number

L, subshell (shape of orbital)

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l=what on s orbital

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l=what on p orbital

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l=what on d orbital

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magnetic quantum number

m(l), orientation of orbital (d- -2 to 2; s= 0, p= -1 to 1)

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l=what on f orbital

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spin quantium number

direction of the spin (+1/2 or -1/2)

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transition metals in electron configuration

s and d orbitals only. also electron is removed from s orbital first

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negative ion

= MORE electrons

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positive ion

= LESS electrons

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atomic radius

smaller left to right, larger top to bottom

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ionization energy

energy required to move one elctron from an atom. higher left to right, lower top to bottom.

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electron affinity

increase left to right, lower top to bottom

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nonpolar covalent

electrons shared equally

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polar covalent

electrons not shared equally

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polar and nonpolar depend on what

electronegativity

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electronegativity

increasing left to right, decreasing top to bottom

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pure covalent number

less than 0.4

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polar covalent number

between 0.4 and 1.8

ionic number

greater than 1.8

formal charge

valence electrons- (lone pair electrions + 1/2 bonding electrons)

bond order

sum of indiviedual bond orders/ mumber of bond groups

individual bond order

#of bonds connecting atoms

breaking bonds ____ energy

requires (endothermic)

building bonds ____ energy

releases (exothermic)

size pattern

decreases up and decreases left to right

ionic bond strength

1. charge 2. size

charge ionic bond strength

higher charge= higher bond strength (aka lattice energy)

size bond strength

smaller ion = higher bond strength (lattice energy)

____ bonds = higher melting points

stronger

covalent bond strength

1. # of bonds 2. size

reaction enthalpy

Ebonds broken- Ebonds formed

bonds broken are the ____

reactants

bonds formed are the____

products

more bonds = ____ length

shorter

electronic geometry-2 bonds + lone pairs

linear, 180 angle

electronic geometry-3 bonds + lone pairs

trigonal planar, 120 degrees

electronic geometry- 4 bonds + lone pairs

tetrahedral, all 109.5 degrees

electronic geometry- 5 bonds + lone pairs

trigonal bipyramidal , angles of 90 or 120

electronic geometry- 6 bonds + lone pairs

octahedral, angles 90 or 180

trigonal planar with 1 lone pair

bent, angles left are less than 120 degrees

tetrahedral one lone pair

trigonal pyramid, angles left are less than 109

tetrahedral with 2 lone pairs

bent, but angles are less than 109

trigonal bipyramid, one lone pair

seesaw, angles of less than 90 (straight to bottom) and less than 120 (between bottom 2)

trigonal bipyramid, 2 lone pairs

t shape, angles of less than 90 degrees

trigonal bipyramid, 3 lone pairs

linear, 180 degrees

octahedral, 1 lone pair

square pyramid, ALL angles less than 90

octahedral, 2 lone pair

square planar, 90 degrees

octahedral, 3 lone pair

t shaped, less than 90 degrees

octahedral, 4 lone pair

linear, 180 degrees

localized

electrons in bonds. they take up less space because they are shared

delocalized

lone pair electrons. they take more space because they are not shared

angle distortion

lone pairs on central atoms will distort bond angles

when is a it polar

when EG and MG are NOT the same. (this means there IS a dipole moment), OR if there are different bond types, it is also polar

when is it nonpolar

when EG and MG are the same (no dipole moment)

be able to write the s, d, and p orbitals

s on left (1 on top + helium on left), d in middle (3 on top (NOT 4)), p on right, (2 on top- not including helium)

EG= linear, what is hybridization?

EG= trigonal planar, what is hybridization?

sp2

EG= tetrahedral, what is hybridization?

sp3

EG= trigonal bipyramidal, what is hybridization?

sp3d

EG= octahedral, what is hybridization?

sp3d2

hybrid orbital what do you do

the hybridization = the # of regions (i.e. sp2= 3 regions), then valence electrons = the spins (start with up, then go back with the extras as down spins)

single bond (sigma and pi)

sigma bond

double bond (sigma and pi)

1 sigma, 1 pi

triple bond (sigma and pi)

1 sigma and 2 pi

when can molecules rotate?

only in a single bond

energy units

J/photon

energy symbol

change in E

wavelength

^ | (the weird one)

frequency

when does it come out of s orbital first?

transition metals

what takes 1 s and 10 d (the exceptions)

Cr and Cu

shielding

electrons are repelled by other electrons in lower shells (so when its up vs down idk)

the more negative energy is...

the higher electron affinity it has

a high electron affinity has ____ energy value

negative