Chemistry Chapter 5 Flashcards
(96 cards)
1
Q
what year did the international congress of chemistry agree on method of determining and standardizing atomic mass
A
1860
2
Q
who organized elements in order of increasing atomic mass; found elements had similar properties at regular intervals
left empty spaces for elements not yet discovered at his time
A
Medelev
3
Q
what are elements grouped together in ?
A
families
4
Q
who and what year did a scientist determine atomic numbers for elements and arranged the periodic table according to atomic number
A
1911 and Mosely
5
Q
the physical and chemical properties of the elements are functions of their atomic numbers
A
periodic law
6
Q
arrangement of elements in order of their atomic numbers so that elements with similar properties fall in the same group
A
the modern periodic table
7
Q
discovery and synthesis of new elements
A
modern additions to the periodic table
8
Q
unreactive elements in our atmosphere
A
noble gases
9
Q
group 1 and 2 elements are in what block?
A
s- block
10
Q
alkali metals
A
s block
11
Q
alkali earth metals
A
s block
12
Q
Li, Na, K, Rb, Cs, Fr
A
group 1 alkali metals
13
Q
all soft, silvery metals
A
group 1 alkali metals
14
Q
melting point> boiling point of water
A
group 1 alkali metals
15
Q
one electron in outer shell
A
group 1 alkali metals
16
Q
very reactive (not found free in nature)
A
group 1 alkali metals
17
Q
Be, Mg, Ca, Sr, Ba, Ra
A
group 2 alkali earth metals
18
Q
all silvery metals but harder and stronger than another group
A
group 2 alkali earth metals
19
Q
two electrons in outer shell
A
group 2 alkali earth metals
20
Q
re-activity
A
group 2 alkali earth metals
21
Q
what block is group 3-12
A
d-block elements
22
Q
what are group 3-12 called
A
transition elements and d-block elements
23
Q
all metals
A
groups 3-12 transition metals
24
Q
have properties of metals
- less reactive
- high luster
- good conductivity
A
groups 3-12 transition metals
25
what block is group 13-18
p-block elements
26
properties vary
group 13-18 p-block
27
some non-metals
some metalloids
some metals
group 13-18 p-block
28
what block are halogens in?
p-block
29
what group is halogens in?
group 17
30
F, Cl, Br, At
group 17 halogens
31
all non-metals
group 17 halogens
32
very reactive
group 17 halogens
33
7 electrons in outer shell
group 17 halogens
34
what block is noble gases in?
p-block
35
what group are the noble gases in
group 18
36
He, Ar, Kr, Xe, Rn
group 18 noble gases
37
all non-metals and gases
group 18 noble gases
38
8 electrons in outer shell/except helium
group 18 noble gases
39
non-reactive
group 18 noble gases
40
what block is the lanthanide series in?
f-block
41
What block is the actinide series in?
f-block
42
contains radioactive elements
f-block actinide series
43
natural and man-made
f-block actinide series
44
atomic radii as a periodic property
- _______ across periods due to ___________ positive charge of the nuclei
- _______ down a group due to ___________ number of levels
decreases, increasing
| increase, increasing
45
minimum amount of energy to remove an electron
| A+energy-->Apositive+electron
ionization energy
46
loosing electron makes ion more _____
positive
47
ionization energy as a periodic property:
- ______ across the periods due to _____ nuclear change
- ______ down the column due to distance from the nucleus
increases, increasing
| decreases
48
removing electron from positive ions
- each _____ electron removed from an ion feels an _______ stronger effective nuclear charge-> ionization energy _____
- a _____ ionization energy ______ occurs when a electron is removed from an inner, stable level
successive, increasing, increases
| large, increase
49
energy released when an atom acquires an electron
| A+electron-->Anegative+energy
electron affinity
50
electron affinity
| when energy is released=__________ value
negative
51
- values become ____ negative across the periods
| - values become ____ negative down a column
more
| less
52
positive ion
cation
53
negative ion
anion
54
cation: _____ radius compared to atom due to loss of outer shell electron and _____ nuclear pull
smaller, increased
55
anion: _____ radius compared to atom due to ______ nuclear pull and ______ electron cloud
large, decreased, increasing
56
of electrons in outer shell
valence electrons
57
```
valence electrons
group 1 =?
group 2=?
group 13=?
group 14=?
group 15=?
group 16=?
group 17=?
group 18=?
```
```
1
2
3
4
5
6
7
8 (except He)
```
58
measure of the ability of an atom in a compound to attract electrons
scale=0-4
0=____ ability to attract
4=____ ability to attract
electronegativity
lowest
greatest
59
electronegativity
____ across the period
____ down the column
increases
| decrease
60
Mendeleev organized the chemical elements based on their
properties
61
A horizontal row in the period table is called a
period
62
the physical and chemical properties of the elements are functions of their atomic number
periodic law
63
An element with the general electron configuration ns^2np^1 for its outermost electrons would be in group
13
64
When a carbon atom is in its ground state, how many electrons does it have in its outermost shell?
4
65
Which of the following elements is most similar in behavior to calcium?
a. magnesium
b. sodium
c. sulfur
d. chlorine
magnesium
66
Which periodic group or family of elements is not correctly matched with its common family name?
a. Group 2: alkaline-earth metals
b. Group 3: alkali metals
c. Group 17: halogens
d. Group 18: noble gases
alkali metals
67
the electron configurations of main group elements end in
s and p orbitals
68
Which of the following elements is a transition metal?
a. calcium
b. iron
c. sodium
d. sulfur
iron
69
all the alkali metal elements are found on the periodic table in
group 1
70
a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called
electronegativity
71
which of the following elements has the greatest atomic radius?
a. Al
b. S
c. Si
d. C
Al
| largersmaller
72
which of the following elements has the lowest electronegativity
a. C
b. F
c. Li
d. O
Li
| lower--electronegativity-->higher
73
which of the following elements has the greatest ionization energy?
a. Ga
b. K
c. Bi
d. As
As
| low--->ionization--->higher
74
which of the following elemnts has an electron affinity of 0kJ/m
a. Br
b. As
c. Ar
d. I
Ar
75
elements have full outer energy levels when they are in the ground state
noble gases
76
in which period is an element that has the electron configuration 1s^2 2s^2 2s^6 3s^2 3p^6 3d^10 4s^2 4p^1
period 4
77
which of the following elements is not a metal?
a. H
b. K
c. Na
d. Fr
H
78
for atoms of p-block elements, the total number of electrons in the highest occupied level is equal to the...
group number minus 10
79
as electrons add to s and p sublevels in the same main energy level they are pulled closer to the more highly charged nucleus, causing
atomic radii to decrease in size
80
which electron configuration would result in the largest negative electron affinity?
a. He 2s^1
b. He 2s^2 2p^2
c. He 2s^2 2p^3
d. He 2s^2 2p^5
He2s^2 2p^5
81
In forming an ion, from which sublevel would an atom of nickel lose electrons first?
4s
82
which one of the following groups contains atoms that, in compounds, have the lowest attraction for electrons
a. group 1
b. group 2
c. group 16
d. group 17
group 1
83
which ionization energy is generally the largest
fourth ionization energy
84
the metalloids are located on the period table between
nonmetals and metals
85
Name the element in group 1 with the most negative (less positive) electron affinity
Li
86
Name the element in Group 17 with the lowest ionization energy
At
87
Name the element in period 2 with the largest atomic radius
Li
88
Name the element in group 15 with the smallest electronegativity
Bi
89
Name the element in period 3 most likely to form an ion with a 2+ charge
Mg
90
electron affinity values tend to become more or less negative?
more
91
ionization energy values tend to become larger or smaller
larger
92
atomic radii tend to become larger or smaller
smaller
93
how will the radius of a magnesium atom compare to the radius of the magnesium ion (Mg+2), explain your answer
Mg>Mg+2
94
what does ionization energy measure
amount of energy required to remove an electron
95
why is F considered to be the most reactive nonmental?
7electrons in outer shell-desperate to get 1 smallest radii- less shells to exert pull on electron highest electronegativity
96
how can you use the periodic table to predict valence eletrons
group 1= 1
group 2= 2
group 13=3
