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Junior 2015-2016 > Chemistry Chapter 5 > Flashcards

Chemistry Chapter 5 Flashcards

1
Q

what year did the international congress of chemistry agree on method of determining and standardizing atomic mass

A

1860

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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

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3
Q

what are elements grouped together in ?

A

families

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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

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5
Q

the physical and chemical properties of the elements are functions of their atomic numbers

A

periodic law

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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

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7
Q

discovery and synthesis of new elements

A

modern additions to the periodic table

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8
Q

unreactive elements in our atmosphere

A

noble gases

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9
Q

group 1 and 2 elements are in what block?

A

s- block

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10
Q

alkali metals

A

s block

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11
Q

alkali earth metals

A

s block

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12
Q

Li, Na, K, Rb, Cs, Fr

A

group 1 alkali metals

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13
Q

all soft, silvery metals

A

group 1 alkali metals

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14
Q

melting point> boiling point of water

A

group 1 alkali metals

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15
Q

one electron in outer shell

A

group 1 alkali metals

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16
Q

very reactive (not found free in nature)

A

group 1 alkali metals

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17
Q

Be, Mg, Ca, Sr, Ba, Ra

A

group 2 alkali earth metals

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18
Q

all silvery metals but harder and stronger than another group

A

group 2 alkali earth metals

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19
Q

two electrons in outer shell

A

group 2 alkali earth metals

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20
Q

re-activity

A

group 2 alkali earth metals

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21
Q

what block is group 3-12

A

d-block elements

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22
Q

what are group 3-12 called

A

transition elements and d-block elements

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23
Q

all metals

A

groups 3-12 transition metals

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24
Q

have properties of metals

  • less reactive
  • high luster
  • good conductivity
A

groups 3-12 transition metals

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25
Q

what block is group 13-18

A

p-block elements

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26
Q

properties vary

A

group 13-18 p-block

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27
Q

some non-metals
some metalloids
some metals

A

group 13-18 p-block

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28
Q

what block are halogens in?

A

p-block

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29
Q

what group is halogens in?

A

group 17

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30
Q

F, Cl, Br, At

A

group 17 halogens

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31
Q

all non-metals

A

group 17 halogens

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32
Q

very reactive

A

group 17 halogens

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33
Q

7 electrons in outer shell

A

group 17 halogens

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34
Q

what block is noble gases in?

A

p-block

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35
Q

what group are the noble gases in

A

group 18

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36
Q

He, Ar, Kr, Xe, Rn

A

group 18 noble gases

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37
Q

all non-metals and gases

A

group 18 noble gases

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38
Q

8 electrons in outer shell/except helium

A

group 18 noble gases

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39
Q

non-reactive

A

group 18 noble gases

40
Q

what block is the lanthanide series in?

A

f-block

41
Q

What block is the actinide series in?

A

f-block

42
Q

contains radioactive elements

A

f-block actinide series

43
Q

natural and man-made

A

f-block actinide series

44
Q

atomic radii as a periodic property

  • _______ across periods due to ___________ positive charge of the nuclei
  • _______ down a group due to ___________ number of levels
A

decreases, increasing

increase, increasing

45
Q

minimum amount of energy to remove an electron

A+energy–>Apositive+electron

A

ionization energy

46
Q

loosing electron makes ion more _____

A

positive

47
Q

ionization energy as a periodic property:

  • ______ across the periods due to _____ nuclear change
  • ______ down the column due to distance from the nucleus
A

increases, increasing

decreases

48
Q

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
A

successive, increasing, increases

large, increase

49
Q

energy released when an atom acquires an electron

A+electron–>Anegative+energy

A

electron affinity

50
Q

electron affinity

when energy is released=__________ value

A

negative

51
Q
  • values become ____ negative across the periods

- values become ____ negative down a column

A

more

less

52
Q

positive ion

A

cation

53
Q

negative ion

A

anion

54
Q

cation: _____ radius compared to atom due to loss of outer shell electron and _____ nuclear pull

A

smaller, increased

55
Q

anion: _____ radius compared to atom due to ______ nuclear pull and ______ electron cloud

A

large, decreased, increasing

56
Q

of electrons in outer shell

A

valence electrons

57
Q 
valence electrons
group 1 =?
group 2=?
group 13=?
group 14=?
group 15=?
group 16=?
group 17=?
group 18=?
A 
1
2
3
4
5
6
7
8 (except He)
58
Q

measure of the ability of an atom in a compound to attract electrons
scale=0-4
0=____ ability to attract
4=____ ability to attract

A

electronegativity
lowest
greatest

59
Q

electronegativity
____ across the period
____ down the column

A

increases

decrease

60
Q

Mendeleev organized the chemical elements based on their

A

properties

61
Q

A horizontal row in the period table is called a

A

period

62
Q

the physical and chemical properties of the elements are functions of their atomic number

A

periodic law

63
Q

An element with the general electron configuration ns^2np^1 for its outermost electrons would be in group

A

13

64
Q

When a carbon atom is in its ground state, how many electrons does it have in its outermost shell?

A

4

65
Q

Which of the following elements is most similar in behavior to calcium?

a. magnesium
b. sodium
c. sulfur
d. chlorine

A

magnesium

66
Q

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

A

alkali metals

67
Q

the electron configurations of main group elements end in

A

s and p orbitals

68
Q

Which of the following elements is a transition metal?

a. calcium
b. iron
c. sodium
d. sulfur

A

iron

69
Q

all the alkali metal elements are found on the periodic table in

A

group 1

70
Q

a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called

A

electronegativity

71
Q

which of the following elements has the greatest atomic radius?

a. Al
b. S
c. Si
d. C

A

Al

largersmaller

72
Q

which of the following elements has the lowest electronegativity

a. C
b. F
c. Li
d. O

A

Li

lower–electronegativity–>higher

73
Q

which of the following elements has the greatest ionization energy?

a. Ga
b. K
c. Bi
d. As

A

As

low—>ionization—>higher

74
Q

which of the following elemnts has an electron affinity of 0kJ/m

a. Br
b. As
c. Ar
d. I

A

Ar

75
Q

elements have full outer energy levels when they are in the ground state

A

noble gases

76
Q

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

A

period 4

77
Q

which of the following elements is not a metal?

a. H
b. K
c. Na
d. Fr

A

H

78
Q

for atoms of p-block elements, the total number of electrons in the highest occupied level is equal to the…

A

group number minus 10

79
Q

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

A

atomic radii to decrease in size

80
Q

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

A

He2s^2 2p^5

81
Q

In forming an ion, from which sublevel would an atom of nickel lose electrons first?

A

4s

82
Q

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

A

group 1

83
Q

which ionization energy is generally the largest

A

fourth ionization energy

84
Q

the metalloids are located on the period table between

A

nonmetals and metals

85
Q

Name the element in group 1 with the most negative (less positive) electron affinity

A

Li

86
Q

Name the element in Group 17 with the lowest ionization energy

A

At

87
Q

Name the element in period 2 with the largest atomic radius

A

Li

88
Q

Name the element in group 15 with the smallest electronegativity

A

Bi

89
Q

Name the element in period 3 most likely to form an ion with a 2+ charge

A

Mg

90
Q

electron affinity values tend to become more or less negative?

A

more

91
Q

ionization energy values tend to become larger or smaller

A

larger

92
Q

atomic radii tend to become larger or smaller

A

smaller

93
Q

how will the radius of a magnesium atom compare to the radius of the magnesium ion (Mg+2), explain your answer

A

Mg>Mg+2

94
Q

what does ionization energy measure

A

amount of energy required to remove an electron

95
Q

why is F considered to be the most reactive nonmental?

A

7electrons in outer shell-desperate to get 1 smallest radii- less shells to exert pull on electron highest electronegativity

96
Q

how can you use the periodic table to predict valence eletrons

A

group 1= 1
group 2= 2
group 13=3

Junior 2015-2016 (15 decks)

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