Final Flashcards

1
Q

effective nuclear charge (Zeff)

A
  • increases from left to right

- stays the same top to bottom(increases slightly)

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2
Q

Core size

A
  • Decreases from left to right

- Increases as descends

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3
Q

Electron affinity

A
  • more negative left to right
  • more positive most positive as descends frst column only
  • -no clear trend in general going down
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4
Q

Melting point

A

GROUP 1A: Decreases as descends

Group 7A: Increases as descends

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5
Q

Density

A

GROUP 1A: Decreases as descends

Group 7A: Increases as descends

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6
Q

Metallic Characteristics

A
  • decreases from left to right

- Increases as descends

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7
Q

ionization energy

-energy needed to remove an electron

A
  • Increases from left to right

- Decreases as descends

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8
Q

Halogens with respect to electron affinity

A

very exothermic electron affinity values
-electron affinity values are more negative for elements that prefer to gain, rather than lose, an electron (negative ions)

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9
Q

boiling part for group 7A

A

-increase as descends

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10
Q

what is true regarding ionization energies

A

they are all endothermic

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11
Q

Elements have a series of ionization energies for removing the first and additional electrons from the atom. Each ionization energy increases for successive electrons being removed. Where will the largest jump in ionization energies occur for aluminum?

A

Aluminum because it has there valence electrons so the fourth, the shell electron will be the hardest to remove

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12
Q

what is the most reactive nonmetal, in fairly extremes circumstances,

A

fluorine

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13
Q

The effective nuclear charge is the amount of charge experienced by an electron taking into account any shielding effects from other electrons. Electrons between the nucleus and the electron of interest cause shielding and reduce the actual charge felt by the electron of interest.

The outermost electron of boron experiences a lower effective nuclear charge than carbon. Why?

A

The nuclear charge increases from boron to carbon, but there is no additional shielding.

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14
Q

what happens as you move down he rows

A

Higher energy levels

-more electronic shells

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15
Q

what happens as you move across the columns

A

more electronic valence shells

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16
Q

how to alkali metals react with halogens

A

diatomic elements that reacts vigorously with sodium metal to produce compounds for example

Br2+2Na–2BrN

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17
Q

size comparison anion, cation, neutral

A

Anion, Neutral, Cation

Biggest——->Smallest

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18
Q

How many covalent bonds are usually formed from the element F

A

1

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19
Q

when is it appropriate to form double or triple bonds in a Less Structure?

A

when the central atom does not have an octet of electrons

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20
Q

How many covalent bonds are usually formed from the element H

A

1

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21
Q

How many covalent bonds usually formed by N

A

3

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22
Q

How many covalent bonds usually formed by O

A

2

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23
Q

How many covalent bonds are usually formed by the element C

A

4

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24
Q

2 electron groups
2 bonding groups
0 lone pairs

A

Electron: linear
Molecular: linear
Angles: 180
Hybridization: sp

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25
Q

3 electron groups
3 bonding groups
0 lone pairs

A

electron: trigonal planar
molecular: trigonal planar
angle: 120
Hybridization: sp2

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26
Q

3 electron groups
2 bonding groups
1 lone pair

A

electron: trigonal planar
molecular: bent
angle: <120
Hybridization: sp2

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27
Q

4 electron groups
4 bonding groups
0 lone pair

A

electron: tetrahedral
molecular: tetrahedral
angel: 109.5
Hybridization: sp3

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28
Q

4 electron groups
3 bonding groups
1 lone pair

A

electron: tetrahedral
molecular: trigonal pyramidal
angle: <109.5
Hybridization: sp3

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29
Q

4 electron groups
2 bonding gropus
2 lone pairs

A

electron: tetrahedral
molecular: bent
angle: «109.5
Hybridization: sp3

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30
Q

5 electron groups
5 bonding groups
0 lone pairs

A

electron: trigonal bipyramidal
Molecular: trigonal bipyramidal
angle 120 equatorial 90 axial
Hybridization: sp3d

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31
Q

5 electron groups
4 bonding groups
1 lone pair

A
electron trigonal bipyramidal
molecular: seesaw
ange: <120 equatorial
<90 axial
Hybridization: sp3d
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32
Q

5 electron groups
3 bonding groups
2 lone pairs

A

electron: trigonal bipyramidal
molecular: t shaped
angle <90
Hybridization: sp3d

33
Q

5 electron groups
2 bonding groups
3 lone pairs

A

electron: trigonal bipyramidal
molecular: linear
angle 180
Hybridization: sp3d

34
Q

6 electron groups
6 bonding groups
0 long pairs

A

electron octahedral
molecular octahedral
angle 90
Hybridzation: sp3d2

35
Q

6 electron groups
5bonding groups
1 lone pair

A

electron octahedral
molecular square pyramidal
angle <90
Hybridzation: sp3d2

36
Q

6 electron groups
4 bonding groups
2 lone pairs

A

electron octahedral
molecular square planar
angle 90
Hybridzation: sp3d2

37
Q

ClF3: polar, non polar, or ionic

A

polar

38
Q

NH3 ionic, polar, non polar

A

polar

39
Q

Li3N ionic, polar, nonpolar

A

ionic

40
Q

C2H4 polar, non polar, or ionic

A

non polar

41
Q

PCl3 polar, non polar, ionic

A

polar

42
Q

H2O polar non polar ionic

A

polar

43
Q

Cl4C polar, non, ionic

A

non polar

44
Q

SF6 polar, non polar, ionic

A

non polar

45
Q

PF5 ionic, polar, non polar,

A

non polar

46
Q

C2H3N. polar non polar ionic

A

polar

47
Q

XeF4 ionic, polar, non polar

A

non polar

48
Q

which element will form the most polar bond with fluorine

A

Boron

49
Q

N2 polar, non polar, ionic

A

non polar

50
Q

general trends in electronegativity values

A

increase from left to right, decrease from top to bottom

51
Q

what type of intermolecular forces are found in H2CO

A

dispersion and dipole-dipole forces

52
Q

Wha types of intermolecular forces are found in CH2Cl2

A

dispersion and dipole-dipole forces

53
Q

London Dispersion force (LDF)

A

present/possible for any atom and all covalent compounds

-polar or non polar

54
Q

Dipole interactions

A

only exist in polar covalent molecules because required to have a permanent dipole

55
Q

Hydrogen bonds

A

special dipole-dipole meets these conditions:

  1. molecule must have H in a very polar bond (H bonded to N,O,F)
  2. neighbor molecules must have a N,O,F (atoms with high electronegativity and lone pairs of electrons)
56
Q

Dipole bonds in liquids vs solids

A

Liquids: attractions and repulsions
solid: only attractions

57
Q

Which bonds are harder to break

A

those with higher boiling point and melting point, therefor a higher LDF

58
Q

MW, LDF, MP, and BP, surface area, and period

A
MW increases
LDF increases
Boiling point Increases
Melting point: increaeses
More surface area
Peroid decreases
59
Q

polarizability

A

ability to “squash manipulate the electronic cloud

60
Q

Low polaralizabeility vs high

A

Low= “hard” low LMF

High=”soft” high LMF

61
Q

CO2 polar or nonpolar

A

non polar

62
Q

CH4 polar or non polar

A

non polar

63
Q

what type of interaction will occur between H2O and Na+

A

ion-dipole forces

64
Q

C+H bonded

A

always non polar

65
Q

same ions/atoms bonded together

A

always non polar

66
Q

BF4 polar or non polar

A

non polar

67
Q

energy levels of bonding and antibonding orbitals?

A

The energy of a bonding orbital is always lower than the energy of the corresponding antibonding orbital.

68
Q

Diamagnetic vs paramagnetic

A

Diamagnetic: all of the electrons are paired

Paramagnetic because it has unpaired electrons

69
Q

What type of orbitals overlap to form the N-H bond in NH3?

A

sp3 of nitrogen and s of hydrogen

70
Q

formula for bond order

A

(electrons in bonding orbitals - electrons anti bonding orbitals)/2

71
Q

bond order definition

A

the number of chemical bonds between a pair of atoms.

72
Q

the energy of a boding orbital is…

A

always lower than th energy of the corresponding anti bonding orbital

73
Q

valence bond theory is based on the idea that

A

electrons in atomic or hybrid orbitals overlap to form bonds

74
Q

the higher the bond order…

A

the more stable the bond

75
Q

how are the number of standard atomic orbitals related to he number of hybrid atomic orbitals

A

they are equal

76
Q

what is hybridization

A

The mathematical combination of standard atomic orbitals to form hybrid atomic orbitals where the number of standard atomic orbitals equals the number of hybrid atomic orbitals

77
Q

what orbitals overlap occur to form triple bond

A

one sigma bond and two pi bonds

78
Q

Which of the properties of a liquid are dependent on the intermolecular attractive forces in the liquid?

A

viscosity, surface tension, density