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chem > Imf prop > Flashcards

Imf prop Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

Trigonal pyramidal

A

one lone pair causes push
three covalent
107 angle

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2
Q

linear

A

2 atoms only or 2 colvalent bonds no lone pair on central atom

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3
Q

tetrahedral

A

0 lone pairs
4 covalent bonds
y can be any atom in 7a or H
angle is 109.5

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4
Q

trigonal planar

A

0 lone pairs
3 covalent bonds
120 angle

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5
Q

bent

A

2 covalent bonds
2 lone pairs
angle 105

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6
Q

Intermolecular forces

A

H bond(H-NOF)
Dipole interaction
London dispersion forces

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7
Q

LDF def

A

an accidental induced dipole b/c of constant motion of the electrons every molecule has the potential to have london disperion forces
weakest IMF1

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8
Q

Dipole interaction Def

A

Between 2 poalr molecules w/no H-NOF

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9
Q

Hydrogen bond

A

between 2 polar molecules containinh H-NOF

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10
Q

what determines the phsycial and chemical of compounds

A

WHat they are made of
strength of bonds
molecular geomertry

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11
Q

Like dissolves

A

like

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12
Q

phases

A

solid liquid gas

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13
Q

high boiling point

A

strong bond

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14
Q

high Melting point

A

strong bond

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15
Q

high surface tension

A

strong bond

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16
Q

high vapor pressure

A

weak bond

17
Q

high heat capacity

A

strong

18
Q

high heat capacity

A

strong

19
Q

bond strength order

A

Network Covalent
Ionic
Covalent
Mettalic

20
Q

stronger bond

A

more effort/energy/work to break it

21
Q

what breaks when ionic is dissolved

A

ionic bonds and lattice crystal 2 breaks into ions

22
Q

what breaks when molecular is disolved

A

IMF break into molecules

23
Q

Network Covalent

A

Stronger then single covalent
charcoal graphie diamonds SiO2 SiC Abestos
Insol
Many covalent bonds rpeating long chains or layers stronfest of all bonds

24
Q

highest vapor pressure

A

covalent

25
Q

ionic finding bondstrength

A
  1. magnitude of charges (add up e-)
  2. larger size if same magnitude
26
Q

metallic finding bondstrength

A
  1. sea of electron sizd ( bigger amount of e- lost)
  2. size greater effective nuclear charge smaller
27
Q

Molecualr comp bondstrenghth

A
  1. compare imf
  2. size- larger= strong bond
28
Q

Ionic compound

A

M&NM
transfer of e-
posititve charge- cation metal
negative charge - anion nonmetal

29
Q

Ionic property

A

crystalline solids at rt
high mp and bp
conduct electricity when molten or aqueous
greatest ionic character

30
Q

Molecular property

A

NM+NM
share e-
do not conduct electricity
solid liquid gasses
low mp and bp

31
Q

polar

A

nonmetals of unequal strength
do not share e- equally
one slightly neg with more electronegativity one slightly pos

32
Q

Nonpolar

A

two nonmetal atoms are the same time and share the bonding electrons equally because they have the same electronegativity

33
Q

Polar Molecule

A

A molecule whos structure has oppositely charged sides witha dipole. High in ionic character due to prtially charged poles on the molecules

34
Q

Nonpolar molecule

A

Either the molecular strucutre has no oppositely charged poles or the poles cancel eachother out
little ionic character

35
Q

Strongest bond

A

covalent bonds molecules do not break apart into smaller particles ithout being involved in chemcial reactions

36
Q

Metallic solid

A

cations held together in a sea of valance electrobs
the larger the sea of electrons the stronger the bond is if 2 metals have the sme charge, then depends on the atomic radii. Smaller metals with fewer occupied levels have greater effective nuclear charge and strong bonds

37
Q

single bond

A

weakest longest
sigma

38
Q

double bond

A

stronger shorter
sigma pi

39
Q

triple bond

A

strongest shortest sigma pi pi

chem (9 decks)

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