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Honors Chem 1320 > Electron Configuration And Lewis Structures > Flashcards

Electron Configuration And Lewis Structures Flashcards

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1
Q

binding energy depends on

A

n and l

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2
Q

difference in binding energy due to having a multi electron system

A

based on z effective, not z

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3
Q

Hunds Rule

A

when e- are added to states if the same energy, a single electron enters each state before a second does

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4
Q

paramagnetic

A

energy state has an unpaired electron

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5
Q

diamagnetic

A

no unpaired electron

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6
Q

most stable electron configurations

A

filled or 1/2 filled

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7
Q

aufbau principle

A

fill energy state 1 at a time, starting with fhe lowest energy

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8
Q

anion

A

ion that gained an electron and has a negative charge

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9
Q

cation

A

ion that lost an electron and is positively charged

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10
Q

transition metals lose what first

A

4s

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11
Q

relationship between IE2 and IE

A

IE2 is always greater than IE

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12
Q

when an ion is by itself charge =

A

oxidation state

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13
Q

isoelectronic

A

same electron configuration

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14
Q

Zeff

A

effective nuclear charge

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15
Q

Zeff trend (and why)

A

▪ increase across periodic table (bc more protons)

▪decrease down periodic table (bc n inc)

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16
Q

ionization energy is always a ______ value

A

positive

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17
Q

ionization energy trends

A

▪inc across periodic table

▪dec down periodic table

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18
Q

Electron affinity

A

ability of an atom to gain electrons

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19
Q

electron affinity = -______

A

change in energy

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20
Q

positive electron affinity means

A

atom wants an electron

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21
Q

electron affinity trends (and why)

A

▪inc across periodic table
▪dec going down
▪bc Zeff

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22
Q

electronegativity

A

the net ability of an atom to attract an electron from another atom

23
Q

electron acceptor

A

atom with high electronegativity

24
Q

electron donor

A

atom with low electronegativity

25
Q

electronegativity trends

A

▪inc across

▪dec down

26
Q

msot electronegative element

A

flourine

27
Q

noble gas electronegativity

A

0

28
Q

atomic radius trend (and why)

A

▪Dec across period table (bc Zeff inc)

▪inc down periodic table (bc n inc)

29
Q

electronegativity inc by what amount across the periodic table?

A

.5

30
Q

difference of electronegativity causes

A

a polar molecule

31
Q

ionic bonds

A

transfer of one or more electrons from one atom to another with a bond

32
Q

ionic bonds are caused by

A

coulombic attraction

33
Q

covalent bonding

A

▪a pair of electrons are shared between 2 atoms

34
Q

on covelnt bond graph, the x intercept =

A

bond length (sharing electrons at a good distance)

35
Q

on covelent binding graph, difference between x intercept and asymptote =

A

dissociation energy

36
Q

dissociation energy

A

energy required to seperate bonded atoms

37
Q

deeper well in covalent bonding graph=

A

stronger bond

38
Q

energy of interaction

A

nuclear-nuclear repulsion + electron-nucleur attraction + electron-electron repulsion

39
Q

polar covalent

A

unequal sharing of electrons between 2 atoms w a different electronegativities

40
Q

difference between electronegativities to form a polar covalent bond

A

.4 < x< 1.7

41
Q

octet rule

A

electrons distributed in such a way that each element is surrounded by 8 electrons

42
Q

coreect lewis structure has the ________ formal charge

A

least complicated

43
Q

if a lewis structure only has single bonds it has no ______

A

resonance structures

44
Q

octet rule exceptions

A

▪odd number of electrons
▪octet deficient molecules
▪valence shell expansion

45
Q

radical species

A

molecules with an unpaired electron

46
Q

valence shell expansion

A

element with n greater than or equal to 3 can have more than 8 electrons around the central atom

47
Q

ionic bonds are between a

A

mental and nonmetal

48
Q

less than an octet most often occurs with the elements

A

▪Boron (B)
▪Beryllium (Be)
▪aluminum (Al)

49
Q

covalent bondimg occurs between

A

2 nonmetals

50
Q

orbital filling exceptions

A

Cr, Cu

51
Q

Cr electron configuration

A

▪6 total electrons
▪4s orbital filled with one
▪3d each filled with one

52
Q

Cu electron configuration

A

▪11 total electrons
▪4s with 1
▪3d completely filled

53
Q

group with the highest electron affinity

A

halides

54
Q

methyl group

A

CH3

Honors Chem 1320 (8 decks)

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