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Chemistry > Periodic Trends > Flashcards

Periodic Trends Flashcards

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0
Q

H - discovered by? Named by?

A

H. Cavendish, Lavoisier

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1
Q

H

A

Colorless, odorless, tasteless, family of its own, simplest element, sometimes placed in groups 1A (metal) or 7A (nonmetal) because can lose/gain one electron and it’s active/diatomic (H2)

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2
Q

H - Haber Process?

A

H reacts with N to form ammonia

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3
Q

When H reacts with a halogen, what does it produce?

A

Acids

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4
Q

Binary H compounds

A

H + active metal = metallic hydrides (react with metals)
H found in abundance in water and fossil fuels
H produced by electrolysis of water, byproduct of oil refining

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5
Q

Group 1A

A

Alkali Metal Family (when these react with water, they form basic things) - Na, Li, K, Rb, Cs, Fr

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6
Q

Describe alkali metals.

A
  1. Most reactive metals
  2. Light
  3. Electrical conductivity
  4. Lustrous (when freshly cut, reacts immediately, then blackens to dark gray)
  5. Soft, low density, cut with pocket knife
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7
Q

Eager to gain or lose one electron? Are they ever found in metallic form in nature?

A

Lose to form a I+ ion

no, never, too reactive

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8
Q

Constituent of table salt

A

Na

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9
Q

Carry electrical signals through nerves and to trigger muscle contractions

A

Na and K

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10
Q

Found in small quantities in tea and coffee

A

Rb

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11
Q

No known uses

A

Fr

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12
Q

Group 2A

A

Alkaline Earth family - Be, Mg, Ca, Sr, Ba, Ra

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13
Q

Describe alkaline earth…

A

Shiny luster under dull gray coating, malleable, heavier, harder, less shiny than 1A, less reactive, form 2+ b/c like to lose 2 valence electrons, reactivity grows as you go down the group

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14
Q

Necessary part of balanced diet (strong bones)

A

Ca

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15
Q

Major use for building materials

A

CaCO(3) - limestone - foundational material in concrete and finishing plaster

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16
Q

Elements responsible for hard water

A

Mg and Ca

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17
Q

Used to treat some specific forms of cancer

A

Ra

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18
Q

Used to produce brilliant colors in fireworks

A

Sr, Mg, and Ba

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19
Q

Used in x-rays of intestinal tract

A

Ba

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20
Q

Element found in Epsom salts

A

Mg

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21
Q

Element found in stomach soothing milk of magnesia (Mg(OH)2)

A

Mg

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22
Q

Transition metals

A

All B groups, heavy, hard, conduct electricity, lustrous, varied chemical properties (Au-Fe)

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23
Q

Only liquid at room temp (B groups)

A

Hg

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24
Q

Trace amounts in human body

A

Fe, Cu, Cr, Mn

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25
Q

Paint

A

Ti

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26
Q

Magnetic by themselves

A

Fe, Cu, Ni

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27
Q

Inner transition metals

A

La and Ac (Lanthanide and Actinide Series)

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28
Q

Actinides

A

Radioactive, U found in nuclear power plants, most are man made, transuranium elements - atomic number > 92

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29
Q

Lanthanide Series

A

Rare earth metals b/c they’re seldom found and difficult to remove from their ores, strongly paramagnetic (weakly attracted to magnetic fields b/c of unpaired electrons)

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30
Q

Group 3A

A

Boron Family (B, Al, Ga, In, Tl), all metals except for Boron which is a metalloid

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31
Q

Excellent semiconductor

A

B

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32
Q

Compound used in glass to aid in thermal expansion to help prevent breakage from rapid temperature changed

A

B

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33
Q

Laundry aid and water softener

A

B

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34
Q

Al

A

High strength and low density, nontoxic nature that is easily machined and highly conductive = very important metal

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35
Q

Most abundant METAL in earth’s crust

A

Al

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36
Q

Bauxite

A

Al, O, and H form this ore (precious metal because hard to separate)

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37
Q

Crown jewel in England before process of extracting this element from it’s ore was common

A

Al

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38
Q

Group 4A

A

C (nonmetal), Si and Ge (metalloids), and Sn and Pb (metals), wide range of properties

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39
Q

Could be in a family by itself

A

C

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40
Q

One of the most important elements

A

C

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41
Q

Basis of organic chemistry

A

C

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42
Q

From Latin, Carbo

A

C

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43
Q

2nd occurring forms

A

Diamond and graphite (more pressure = more condensed)

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44
Q

28% of the earth’s crust (does not occur alone)

A

Si

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45
Q

Basis of rocks, soils, clays, and sands

A

Si

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46
Q

Does not react with air, water, or acids at low temps

A

Si

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47
Q

Used in filters to strain out organic impurities

A

C

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48
Q

Vital in microchips - why?

A

Si - allows flow of e- and semiconductor so doesn’t let it get too hot

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49
Q

Bronze

A

Sn + Cu

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50
Q

Low melting point

A

Ge

51
Q

Used in ammunition and smoldering of stained glass

A

Pb

52
Q

Group 5A

A

N and P (non metals), As and Sb metalloids, Bi (metal), most dramatic changes in properties

53
Q

Named “Azote”

A

N - meaning lifeless because cannot support life

54
Q

N

A

Discovered by Rutherford, colorless, tasteless, and odorless, diatomic gas

55
Q

Glows in the dark

A

P

56
Q

Named for Greek (light bearer)

A

P

57
Q

78% of earth’s atmosphere

A

N

58
Q

Exists in 4 colors depending on atom arrangement

A

P (red, white, yellow, and black)

59
Q

Triple bonds naturally

A

N - difficult to split, releases lots of energy

60
Q

Highly reactive especially with oxygen

A

P

61
Q

Plants and animals need constant supply, found in soil

A

N

62
Q

Used in match heads

A

P

63
Q

Used in fertilizers in liquid form

A

N

64
Q

Laughing gas and smog pollutants

A

N

65
Q

Used in poison and glass mfg.

A

As

66
Q

Group 6A

A

O, S, Se, Te, Po

67
Q

O

A

Gaseous nonmetal, discovered by Priestley, colorless, odorless, tasteless, combustion, life, rust

68
Q

Called brimstone in the Bible

A

S (several forms but usually a yellow solid)

69
Q

O3

A

Ozone, forms near upper atmosphere, 3 O atoms bonded together to protect us from ultraviolet rays from the sun

70
Q

O2

A

One of the most reactive elements, form compounds called oxides (compounds with O)

71
Q

Sulfides

A

Compounds with S, reactive

72
Q

Component of acid rain

A

S (sulfuric acid)

73
Q

Workhorse of chemical industry

A

Components of sulfuric acid

74
Q

Photocopying

A

Se

75
Q

Acne/eczema/dandruff/skin disease

A

Se

76
Q

Glass tinting

A

Te

77
Q

Printing and thermoelectric power source for satellites

A

Po

78
Q

Groups 7A

A

Halogens (F, Cl, Br, I, At), vary from light to dark-colored gases except Br (liquid) and I (solid), most reactive nonmetals, bad odor, difficult to find pure in nature (want to gain one electron)

79
Q

Highest electronegativity

A

F

80
Q

Salts

A

Halogen + active metals

81
Q

Named for Greek word iodes

A

I (violet)

82
Q

Named for Greek word bromus

A

Br (stench), poisonous, irritating, pungent vapor

83
Q

Most reactive halogen

A

F (one of last discovered because so reactive)

84
Q

Greenish gas

A

Cl

85
Q

Only metallic in halogen family

A

At (unstable, highly radioactive, no stable isotopes)

86
Q

Compounds resist tooth decay

A

F

87
Q

In Teflon

A

F

88
Q

In bleach

A

Cl

89
Q

Component of table salt

A

Cl

90
Q

Lack of it causes stunted growth and goiter

A

I (lack of it in thyroid gland)

91
Q

Used with alcohol as disinfectant

A

I

92
Q

Group 8A

A

Noble gases (He, Ne, Ar, Kr, Xe, Rn), colorless, odorless, tasteless gases, not very reactive (must be forced because they have all 8 valence electrons)

93
Q

Named for Greek word Neos

A

Ne (new)

94
Q

Used to lift air balloons

A

He

95
Q

Deep sea divers used to dilate N2 in air they breathe

A

He

96
Q

Colored lights

A

Ne, Kr, and Xe

97
Q

Post transition metal semiconductor

A

Metalloid

98
Q

Bridge relationship

A

2 metals that are close to each other share properties

100
Q

Electrostatic attractions

A

Coulombic attraction (attraction of oppositely charged particles)

101
Q

Lavoisier

A

“Father of Chemistry”, first list of 30 substances he thought were elements

102
Q

Döbereiner

A

list of elements based on triads (groups of 3 who had similar properties but then turned into groups of 4 and 5)

103
Q

periodicity

A

repetition of property on a regular basis

104
Q

John Newland

A

arranged everything by atomic mass, groups of 8 (“law of octaves”), every 8th element repeats property (included transition elements) - arranged on music sheets

105
Q

Dmitri I. Mendeleev

A

developed the periodic table by arranging elements by atomic mass, included transition elements, when things didn’t fit, he left blanks

106
Q

Lothar Meyer

A

identical table but Mendeleev’s came out first so didn’t get credit

107
Q

Henry Moseley

A

changed the periodic table to atomic number and now elements fit

108
Q

periodic law

A

properties of elements vary with their atomic umber in a systematic way

109
Q

transuranium elements

A

atomic number > 92, exist up to element 118 (some not found yet so three letter symbols)

110
Q

family/group

A

vertical section on periodic table

111
Q

period/series

A

horizontal section on table, equal to energy of s and p sub-levels, one greater to the energy level for the d sub-level

112
Q

North American Convention

A

s and p = A

d and f = B

113
Q

European Convention

A

1-8A, then B’s

114
Q

IUPAC Convention

A

1-18

115
Q

metals

A

left and middle of table, solid, shiny, ductile, malleable, conduct heat and electricity, like to lose electrons in chemical reactions

116
Q

metalloids

A

an element whose properties lie between those of metals and nonmetals, brittle not malleable, do not conduct heat

117
Q

nonmetals

A

gases/soft and crumbly solids, gain electrons in chemical reactions

118
Q

noble gases

A

8A (forced to bond) - full outer shell

119
Q

post-transition metals

A

before metalloids, after d sub-level

120
Q

atomic radius

A

distance from the nucleus to the outermost electron, increases from top to bottom, bc of higher electron levels, decreases from left to right bc if there are more protons, they will have a greater force of attraction pulling the electrons closer

121
Q

ionic radius

A

atoms that lose outer electrons have smaller positive ions (metals), atoms that gain outer electrons have larger negative ions (nonmetals)

122
Q

ionization energy

A

the electron “rip off”, the minimum amount of energy necessary to remove the outermost electron, increases from left to right, decreases from top to bottom

123
Q

electron affinity

A

energy associated with addition of electron to gaseous atom, follows Coulombic attraction, negative ion

124
Q

electronegativity

A

.7 - 4.0 scale, F = 4.0, Fr = .7, measure of tendency of an atom’s nucleus to attract bonded electrons, follows Coulombic attraction

125
Q

Who created an electronegativity table?

A

Linus Pauling

Chemistry (5 decks)

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