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Chemistry 11 > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

Protons have a _ charge

A

Positive

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2
Q

The number of protons is equal to

A

Atomic number

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3
Q

What charge do neutrons have

A

Neutral

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4
Q

What is the number of neutrons equal

A

Atomic mass - atomic #

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5
Q

What is outside the nucleus and what charge do they have

A

Electrons

Negative

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6
Q

Do atoms have a charge

A

No they are neutral

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7
Q

of Electrons are equal to?

A

of protons

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8
Q

Do ions have a charge

A

Yes

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9
Q

For ions the # of _________ is not equal to the ____________

A

Electrons

Protons

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10
Q

What is the name of negative ions

A

Anions

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11
Q

For anions

are the the # of electrons higher or lower and why

A

Higher than the atomic number

Gain electrons

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12
Q

What are positive ions called

A

Cations

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13
Q

For cations

Are the number of electrons higher or lower and why

A

Lower than the atomic #

They lose electrons

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14
Q 
Is 31P a
Atom or ion
# of protons
# of neutrons
# of electrons
A

Atom
15
16
15

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15
Q 
Is 32S a
Atom or ion
# of protons
# of neutrons
# of electrons
A

Atom
16
16
16

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16
Q 
Is 35Cl- a
Atom or ion
# of protons
# of neutrons
# of electrons
A

Ion
17
18
18

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17
Q

What does isoelectronic mean

A

Same # of electrons

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18
Q

Give 3 examples of ions that are isoelectronic with argon

A 
Ar
Ti4+
Ca+2
K+
Cl-
S2-
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19
Q

How many protons does a potassium ion have?

A

19

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20
Q

How many electrons does an oxygen atom have?

A

8

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21
Q

How many electrons does a calcium ion have

A

18

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22
Q

Isotopes element differ in what 3 things

A

Neutrons
Mass
Properties

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23
Q

What is the relative amount of each isotope called

A

Isotopic abundance

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24
Q

The values of each isotope are used to calculate what?

A

Average atomic mass

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25
Q

What is the formula for AAM

A

(%A)(massA) + (%B)(massB)+……

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26
Q

How many electrons does the first layer hold

A

2

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27
Q

How many do the 2nd and 3rd hold

A

8

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28
Q

The proton equal what

A

of electron layers (atomic #)

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29
Q

The number of valence electrons is equal to what

A

Column, family, group #

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30
Q

Sulfer has ____ valence electrons ____ layers of electrons.

A

6

3

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31
Q

What are two ways you can a stable octet

A

Gain electrons to full outer layer

Lose all valence electrons

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32
Q

Elements that have less than 4 valence electrons do what, why and what do they form

A

Lose electrons

Forming cations with a positive charge

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33
Q

Elements that have more than 4 valence electrons do what, why and what do they form

A

Gain electrons
Forming anions with a negative charge
Expect the noble gases

34
Q

Will an element with more layers of electrons gain electrons more easily than an element with fewer layers?

A

No. An element with fewer layers of electrons gains electrons more readily because they are closer to the nucleus creating a greater attraction.

35
Q

Will sulphur gain or lose electron? How many?

A

Gain 2

36
Q

Will aluminium gain or lose electron? How many?

A

Lose 3

37
Q

Which will lose electrons more easily Ba or Ca and why

A

Ba: more layers, less attraction, easier to remove

38
Q

Which will gain electrons more readily: S or Se?

A

Sulphur

  • both have 6 valence electrons
  • S has fewer layers
  • closer to nucleus = easier to gain electrons
39
Q

Which will lose electrons more readily: Na or Fr

A
  • both have 1 valence electron
  • Fr has more layers making the attraction weaker
  • further from nucleus
  • easier to lose electrons
40
Q

What is ionization energy the measure of

A

Energy needed to remove outermost electron

41
Q

What does a high IE value mean

A

Hard to remove electron

42
Q

What does a low IE value mean

A

Easy to remove electron

43
Q

What happens to IE as you go down a group (5)

A

IE decreases

  • more layers
  • less attraction
  • easier to remove
  • low IE
44
Q

What happens to IE when you go across a period (left to right)

A

IE increases

  • valence electrons increase
  • harder to remove
  • more attraction
  • higher IE
45
Q

Which element has highest IE

A

HE

46
Q

Which has a lower IE: Ne or O?

A

O

47
Q

What is electron affinity

A

Measure of the energy involved when an electron is gained

48
Q

What does a higher EA value mean

A

More attraction for the electron

49
Q

What happens to EA when you go down a group

A

EA decreases

  • less attraction for valence electrons to the nucleus
  • harder to gain
  • more layers
50
Q

What happens when you go across a period

A

EA increases

- except for nobles (already full)

51
Q

Which element has the highest EA

A

F

52
Q

Which has a higher EA: Ne or O?

A

O

53
Q

What does the nucleus contain

A

Protons and neutrons

54
Q

What happens to atomic radius as you move down the group

A

Radius increases

- the more layers the larger the radius

55
Q

What happens to atomic radius as you move across a period

A

Radius decreases across periods protons increased drawing them in closer this is called effective nuclear charge

56
Q

What is special about ionic radius for cations

A

Positively charged
Lose layers
Therefore they are much smaller

57
Q

What is special about ionic radius for anions

A

Negatively charged
Gain electrons
Therefore bigger

58
Q

What needs to happen in order for metals to react

A

Give away electrons

59
Q

How do you tell how reactive a metal is

A

The easier to give electrons the more reactive the metal is

60
Q

What happens to metal reactivity when you move down a group

A

Metal Reactivity increases

  • more layers
  • less attraction
  • easier to remove
  • more reactive
61
Q

What happens to metals when you move across a period

A

Metal reactivity decreases

  • fewer electrons
  • harder to give away
62
Q

Arrange from largest to smallest

Ba,Be,Cl,B,C,Ca,Br

A

Ba,Ca,Br,Cl,Be,B,C

63
Q

What is the most reactive metal

A

Fr

64
Q

Which is less reactive. Al or Na?

A

Al

65
Q

What needs to happen for non metal to reactive

A

They need to gain electrons

66
Q

What happens when it is easy for non metal to gain electrons

A

They become very reactive

67
Q

What happens when you move down a group for reactivity of none metals

A

Less Reactive

  • reactivity decreases
  • more layers
  • less attraction
  • harder to gain electrons
68
Q

What happens to non-metal reactivity as you move across a peeiod

A

Reactivity increases

Except nobles

69
Q

What is the most reactive non-metal

A

F

70
Q

Which is less reactive: Cl or Ar?

A

At

71
Q

Which element is more reactive N or P? why?

A

Nitrogen

  • as you move down a group it become less reactive
  • more layers
  • less attraction
72
Q

Which element has a smaller atomic radius: Si or S? Why?

A

Silicon

  • as you move across atomic radius decreases
  • effective nuclear charge
73
Q

What is electronegativity

A

Measure of an atoms ability to attract electrons in a bond

74
Q

What is true about electronegativity

A

The higher the value the higher the attraction

75
Q

Fluorine has the highest value, why?

A
  • 2 layers
  • 7 valence electrons
  • really want that last electron
76
Q

Why don’t nobles have electronegativity values

A
  • noble gases have 8 valence electrons and don’t want anymore
77
Q

What does electronegativity help us determine

A

Type of bond being formed

78
Q

What happens when a transfer of electrons occur and what numbers on the scale

A

Higher value gets the electrons
Results in ions
3.3-1.7

79
Q

What results in a polar bond

A

Can’t take electron completely
Unequal sharing occurs
1.4-0.4

80
Q

What results in non-polar bond

A

Equal sharing

0.4-0.0

81
Q

Find bond between Na and F

A

EN=3.1
Ionic
Fluorine get e—

82
Q

Find bond between C and O

A

EN=0.8

Polar

Chemistry 11 (3 decks)

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