Unit 1 Flashcards
(82 cards)
1
Q
Protons have a _ charge
A
Positive
2
Q
The number of protons is equal to
A
Atomic number
3
Q
What charge do neutrons have
A
Neutral
4
Q
What is the number of neutrons equal
A
Atomic mass - atomic #
5
Q
What is outside the nucleus and what charge do they have
A
Electrons
Negative
6
Q
Do atoms have a charge
A
No they are neutral
7
Q
of Electrons are equal to?
A
of protons
8
Q
Do ions have a charge
A
Yes
9
Q
For ions the # of _________ is not equal to the ____________
A
Electrons
Protons
10
Q
What is the name of negative ions
A
Anions
11
Q
For anions
are the the # of electrons higher or lower and why
A
Higher than the atomic number
Gain electrons
12
Q
What are positive ions called
A
Cations
13
Q
For cations
Are the number of electrons higher or lower and why
A
Lower than the atomic #
They lose electrons
14
Q
Is 31P a Atom or ion # of protons # of neutrons # of electrons
A
Atom
15
16
15
15
Q
Is 32S a Atom or ion # of protons # of neutrons # of electrons
A
Atom
16
16
16
16
Q
Is 35Cl- a Atom or ion # of protons # of neutrons # of electrons
A
Ion
17
18
18
17
Q
What does isoelectronic mean
A
Same # of electrons
18
Q
Give 3 examples of ions that are isoelectronic with argon
A
Ar Ti4+ Ca+2 K+ Cl- S2-
19
Q
How many protons does a potassium ion have?
A
19
20
Q
How many electrons does an oxygen atom have?
A
8
21
Q
How many electrons does a calcium ion have
A
18
22
Q
Isotopes element differ in what 3 things
A
Neutrons
Mass
Properties
23
Q
What is the relative amount of each isotope called
A
Isotopic abundance
24
Q
The values of each isotope are used to calculate what?
A
Average atomic mass
25
What is the formula for AAM
(%A)(massA) + (%B)(massB)+......
26
How many electrons does the first layer hold
2
27
How many do the 2nd and 3rd hold
8
28
The proton equal what
of electron layers (atomic #)
29
The number of valence electrons is equal to what
Column, family, group #
30
Sulfer has ____ valence electrons ____ layers of electrons.
6
| 3
31
What are two ways you can a stable octet
Gain electrons to full outer layer
| Lose all valence electrons
32
Elements that have less than 4 valence electrons do what, why and what do they form
Lose electrons
| Forming cations with a positive charge
33
Elements that have more than 4 valence electrons do what, why and what do they form
Gain electrons
Forming anions with a negative charge
Expect the noble gases
34
Will an element with more layers of electrons gain electrons more easily than an element with fewer layers?
No. An element with fewer layers of electrons gains electrons more readily because they are closer to the nucleus creating a greater attraction.
35
Will sulphur gain or lose electron? How many?
Gain 2
36
Will aluminium gain or lose electron? How many?
Lose 3
37
Which will lose electrons more easily Ba or Ca and why
Ba: more layers, less attraction, easier to remove
38
Which will gain electrons more readily: S or Se?
Sulphur
- both have 6 valence electrons
- S has fewer layers
- closer to nucleus = easier to gain electrons
39
Which will lose electrons more readily: Na or Fr
- both have 1 valence electron
- Fr has more layers making the attraction weaker
- further from nucleus
- easier to lose electrons
40
What is ionization energy the measure of
Energy needed to remove outermost electron
41
What does a high IE value mean
Hard to remove electron
42
What does a low IE value mean
Easy to remove electron
43
What happens to IE as you go down a group (5)
IE decreases
- more layers
- less attraction
- easier to remove
- low IE
44
What happens to IE when you go across a period (left to right)
IE increases
- valence electrons increase
- harder to remove
- more attraction
- higher IE
45
Which element has highest IE
HE
46
Which has a lower IE: Ne or O?
O
47
What is electron affinity
Measure of the energy involved when an electron is gained
48
What does a higher EA value mean
More attraction for the electron
49
What happens to EA when you go down a group
EA decreases
- less attraction for valence electrons to the nucleus
- harder to gain
- more layers
50
What happens when you go across a period
EA increases
| - except for nobles (already full)
51
Which element has the highest EA
F
52
Which has a higher EA: Ne or O?
O
53
What does the nucleus contain
Protons and neutrons
54
What happens to atomic radius as you move down the group
Radius increases
| - the more layers the larger the radius
55
What happens to atomic radius as you move across a period
Radius decreases across periods protons increased drawing them in closer this is called effective nuclear charge
56
What is special about ionic radius for cations
Positively charged
Lose layers
Therefore they are much smaller
57
What is special about ionic radius for anions
Negatively charged
Gain electrons
Therefore bigger
58
What needs to happen in order for metals to react
Give away electrons
59
How do you tell how reactive a metal is
The easier to give electrons the more reactive the metal is
60
What happens to metal reactivity when you move down a group
Metal Reactivity increases
- more layers
- less attraction
- easier to remove
- more reactive
61
What happens to metals when you move across a period
Metal reactivity decreases
- fewer electrons
- harder to give away
62
Arrange from largest to smallest
| Ba,Be,Cl,B,C,Ca,Br
Ba,Ca,Br,Cl,Be,B,C
63
What is the most reactive metal
Fr
64
Which is less reactive. Al or Na?
Al
65
What needs to happen for non metal to reactive
They need to gain electrons
66
What happens when it is easy for non metal to gain electrons
They become very reactive
67
What happens when you move down a group for reactivity of none metals
Less Reactive
- reactivity decreases
- more layers
- less attraction
- harder to gain electrons
68
What happens to non-metal reactivity as you move across a peeiod
Reactivity increases
| Except nobles
69
What is the most reactive non-metal
F
70
Which is less reactive: Cl or Ar?
At
71
Which element is more reactive N or P? why?
Nitrogen
- as you move down a group it become less reactive
- more layers
- less attraction
72
Which element has a smaller atomic radius: Si or S? Why?
Silicon
- as you move across atomic radius decreases
- effective nuclear charge
73
What is electronegativity
Measure of an atoms ability to attract electrons in a bond
74
What is true about electronegativity
The higher the value the higher the attraction
75
Fluorine has the highest value, why?
- 2 layers
- 7 valence electrons
- really want that last electron
76
Why don't nobles have electronegativity values
- noble gases have 8 valence electrons and don't want anymore
77
What does electronegativity help us determine
Type of bond being formed
78
What happens when a transfer of electrons occur and what numbers on the scale
Higher value gets the electrons
Results in ions
3.3-1.7
79
What results in a polar bond
Can't take electron completely
Unequal sharing occurs
1.4-0.4
80
What results in non-polar bond
Equal sharing
| 0.4-0.0
81
Find bond between Na and F
EN=3.1
Ionic
Fluorine get eā
82
Find bond between C and O
EN=0.8
| Polar
