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AP Chemistry > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

electronegativity

A

how badly an atom wants to “hog” electrons

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2
Q

electronegativity trends

A

increases right and decreases down

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3
Q

what is the least and most electronegative elements

A

least- Fr
most-F

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4
Q

which column on the periodic table has no electronegativity?

A

the noble gas family (very last one on the right)

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5
Q

which column on the periodic table has the most electronegativity?

A

the halogen family (the one to the left of the noble gas)

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6
Q

why does electronegativity decrease when you go down?

A

when u go down the atoms get larger and further away from their nucleus so its easier for their electrons to be stolen

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7
Q

nonpolar covalent has what kind of electronegativity difference

A

zero

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8
Q

polar covalent has what kind of electronegativity difference

A

low

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9
Q

ionic bond has what kind of electronegativity difference

A

high

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10
Q

electron affinity

A

how much they “want” electrons

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11
Q

electron affinity trends

A

increases to the right (they want to form octet) and decreases down (they get weaker the lower u go)

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12
Q

cations attract electrons?

A

smaller
more positive force
attracts fewer electrons

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13
Q

anion attract electrons?

A

bigger
less positive force
more electron repulsions (distance between nucleus and electrons)
attracts more electrons

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14
Q

ionization energy

A

energy required to remove an electron
(gas phase)

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15
Q

ionization energy trends

A

increases right
decreases down

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16
Q

elements of the same family=

A

similar properties bc have same number of valence electrons

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17
Q

ionic bonds

A

-mental-nonmetal
-give electrons

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18
Q

covalent bonds

A

-nonmetal-nonmetal
-share electrons

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19
Q

2 types of covalent bonds

A

POLAR
-unequal sharing (bent)

NONPOLAR
-equal sharing

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20
Q

How are alloys formed

A

solution of metal and metal

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21
Q

metalic bonds

A

metal-metal
good conductors
mixture called an alloy

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22
Q

electronegativity difference between nonpolar and polar

A

nonpolar = <0.5
polar = 0.5-1.7

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23
Q

electronegativity difference between ionic

A

> 1.7

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24
Q

another name for ionic bond

A

coulombic or electrostatic attraction

25
Q

properties of ionic substances

A

-form crystals (lattice of positive and negative ions)
-high melting and boiling points
-hard, brittle
-conduct electricity when dissolved or molten
-good insulators as solid

26
Q

what are metallic attractions due to

A

due to multiple metallic cations being attracted to delocalized sea of valence electrons

27
Q

properties of metallic substances

A

-shiny (luster)
-malleable and ductile
-conduct heat and electricity
-metallic oxides are basic and ionic
-lose electrons to form cations

28
Q

properties of covalent molecules

A

-non-lustrous, various colors
-brittle, hard, or soft
-poor conductors
-nonmetallic oxides are acidic and covalent
-form anions by gaining electrons

29
Q

what does “diapole” mean?

A

one side of the compound is more negative or more positive on one side

30
Q

covalent bonds occur at the ___ energy state

A

lowest

bc if theyre too close together the nuclei will repel each other and if too far apart the attraction will not be enough to hold them together

31
Q

bond energy

A

the energy required when breaking a bond or the energy released when bond is formed.

32
Q

larger atomic radii increase the bond length. Larger bond length decrease the ____?

A

bond energy

33
Q

lattice energy

A

the energy to separate ions from ionic compounds

34
Q

lattice energy formula

A

k(Q1Q2)/r

35
Q

Ionic solids

A

-consist of cations and aions
-nonvolatile and have high melting points
-do not conduct electricity
-when melted or dissolved the ions can move freely (which causes electricical conduction)
-soluble in polar
-insoluble in non-polar

36
Q

when ionic radius decreases the attraction___?

A

increases

37
Q

two types of alloys

A

interstitial and substitutional

38
Q

interstitial alloy

A

the atoms added to the metal are small and fit in between the metal atoms in the existing holes (interstices)

39
Q

Substitutional alloy

A

the atoms added to the metal have similar radii so they replace the atoms in the lattice

40
Q

third period with lewis structures

A

able to expand their octet ONLY if theyre the central element

41
Q

Formal charge formula

A

how many electrons its supposed to have- what it has

42
Q

after you find formal charge what do u do

A

pick the one that has the highest number (ex:-1) on the most electronegative element

43
Q

dont forget when u have double, triple whatever bonds to…

A

draw resonance structures!!

44
Q

Valence shell electron-pair repulsion (VSEPR)

A

predicts the geometries of molecules and polyatomic ions (3D stucture)

45
Q

Linear

A

2
180 degrees
sp

46
Q

Trigonal planar

A

3
120 degrees
sp^2

47
Q

Tetrahedral

A

4
109.5 degrees
sp^3

48
Q

overlapping orbitals from a single bonds are known as

A

sigma bonds
(very strong bonds)

49
Q

double and triple bonds are formed from unhybridized p orbital are called

A

pi bonds

50
Q

triple bond contains

A

one sigma and two pi bonds

51
Q

the presence of pi bonds means

A

the bonds are unable to rotate leading to geometric isomers

52
Q

as the number of bonds between two atoms increases, the bond ___?

A

increases in strength but decreases in length

53
Q

pi bonds

A

pull the atoms closer together
(triple and double bonds)

54
Q

triple bonds

A

the strongest and shortest bonds within the highest energy

55
Q

single bonds

A

the longest and weakest bonds with the lowest energy

56
Q

double bonds

A

stronger and shorter and higher in energy than single bonds

57
Q

bond order

A

number of bonds between two atoms

58
Q

Bond order table

A

single 1
double 2
triple 3

59
Q

how do you calculate bond order

(ex- 1 double bond, 2 single bonds)

A

see how many bond categorize there are in ur lewis structure so its between 1 and 2 so find an inbetween that so 1/2 = 1.5

AP Chemistry (9 decks)

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