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chemistry > Untitled Deck > Flashcards

Untitled Deck Flashcards

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1
Q

atomic radius

A

measurement of the space that each element takes up the electron cloud

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2
Q

nonmetals

A

elements that are gases or very brittle, dull-looking solids

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3
Q

noble gases

A

the extremely un-reactive group 18 and elements that are used in lasers and a variety of light bulbs

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4
Q

transition elements

A

elements are classified in groups 3-12

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5
Q

metals

A

elements that give away electrons easily

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6
Q

transition metals

A

an element in groups 3-12 that is contained in d-block and with exceptions

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7
Q

electronegativity

A

indicates the relative ability of its atoms to attract electrons in a chemical bond

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8
Q

octect rule

A

atoms tend to lose, gain, or share electrons in order to acquire 8 valence electrons

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9
Q

halogens

A

group 17 that is comprised of highly reactive elements

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10
Q

inner transition metals

A

a type of group B element that is contained in the f-block of the periodic table and is known by filled outermost orbitals

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11
Q

ionization energy

A

the energy required to remove an electron from a gaseous form

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12
Q

cation

A

ion with a positive charge

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13
Q

alkali earth metal

A

in group 2 and highly reactive metal

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14
Q

transuranium element

A

an element with an atomic number of 93 or greater on the periodic table

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15
Q

energy level (principal)

A

each major energy level in an increased energy of an atom

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16
Q

ion

A

an atom or bonded group of atoms that has a positive charge or a negative charge

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17
Q

orbital (atomic)

A

a three dimensional description of the most likely location of an electron around an atom

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18
Q

actinide series

A

part of the inner transition metals, it is the f-block elements from period 7 that follow the element actinium

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19
Q

electron configuration

A

electron arrangement in an atom

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20
Q

anion

A

ion with a negative charge

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21
Q

lanthanide series

A

part of the inner transition metals, they are extensively used as phospherers-substances that emit light when struck by electrons

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22
Q

Hund’s rule

A

when there’s single electrons with the same spin, it must first occupy each equal-energy orbital before the addition of opposite electron spins

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23
Q

electron dot structure

A

consists of elements symbol surrounded by dots that represent all the valence electrons of an atom

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24
Q

alkali metal

A

group 1 of elements (except hydrogen)

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25
Q

aufbau principle

A

each electron occupies the lowest energy orbital allowed

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26
Q

metalloids

A

combo for both metals and metals-they can be both conductors and nonconductors

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27
Q

periodic law

A

the properties of elements vary periodically with their atomic numbers

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28
Q

sublevel (energy)

A

contained by principal energy levels

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29
Q

group

A

boxes arranged in order by similar traits

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30
Q

valence electrons

A

electrons in the atom’s outermost orbitals

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31
Q

Pauli (exclusion) principle

A

a maximum of z electrons can occupy a single atomic orbital but with opposite spins

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32
Q

periods

A

boxes arranged in order by similar number of protons electrons

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33
Q

Representative elements

A

the elements in groups 1,2, and 13-18 process a wide range of chemical and physical groups.

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34
Q

John Newlands contribution to the periodic table

A

arranged elements by increasing atomic mass

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35
Q

Dmitri Mendeleev contribution to the periodic table

A

found a connection between atomic mass and properties, and predicted the existence and properties of undiscovered elements

36
Q

Henry Mosely contribution to the periodic table

A

he arranged the periodic table based on atomic number

37
Q

Aufbau Principle

A

the lowest level must be filled before moving up

38
Q

Pauli Exclusion Principle

A

If two electrons occupy the same
orbital, they must have opposite spins.

39
Q

Hund’s Rule

A

Electrons will fill an orbital one at a time before pairing up to have the same

40
Q

What is the difference between an orbital, energy level, and sublevel?

A

An energy level is the largest category that defines the periods of the periodic table.

41
Q

Within the energy level there are various sublevels. Some sublevels have multiple orbitals.

A
42
Q

What is electronegativity?

A

how likely an atom is to attract electrons, making it negative. (Electro-negative)

43
Q

How are elements in a group similar and what is the cause of their similarity?

A

They have similar bonding properties, of whether they will take or give electrons because electrons in a group have the same number of valence electrons.

44
Q

What are the typical properties of metals?

A
  • shiny
45
Q

-Malleable

A
46
Q

-Good conductor

A
47
Q

-Solid at room temperature

A
48
Q

-give away electrons more easily

A
49
Q

What are the typical properties of nonmetals?

A

-take electrons more easily

50
Q

-gases or soft

A
51
Q

-Brittle

A
52
Q

-not good conductors

A
53
Q

What are the general properties of metalloids?

A

-mix of metals and nonmetals

54
Q

-Shiny but brittle

A
55
Q

-semiconductors.

A
56
Q

Alkali metals

A

Group 1 elements except for hydrogen, very very reactive, have one valence electron

57
Q

Alkaline earth metals

A

Group 2 elements, very reactive, have 2 valence electrons

58
Q

Halogens

A

Group 17, very very reactive, have 7 valence electrons

59
Q

Noble gases

A

Group 18, very unreactive, have 8 valence electrons

60
Q

Transition metals

A

groups 3-12, variable valence electrons

61
Q

John Newlands

A

Arranged elements by atomic mass; rule of octaves.

62
Q

Dmitri Mendeleev

A

Predicted undiscovered elements based on atomic mass.

63
Q

Henry Mosely

A

Established atomic number; resolved periodic table issues.

64
Q

Valence Electrons Group 2

A

Elements in group 2 have 2 valence electrons.

65
Q

Valence Electrons Group 17

A

Elements in group 17 have 7 valence electrons.

66
Q

Aufbau Principle

A

Electrons fill lower energy orbitals first.

67
Q

Pauli Exclusion Principle

A

Electrons in same orbital must have opposite spins.

68
Q

Hund’s Rule

A

Electrons occupy orbitals singly before pairing.

69
Q

Energy Level

A

Largest category defining periodic table periods.

70
Q

Sublevel

A

Divisions within energy levels containing orbitals.

71
Q

Atomic Radius

A

Measurement of space occupied by electron cloud.

72
Q

Atomic Radius Trend

A

Decreases across a period; increases down a group.

73
Q

Electronegativity

A

Likelihood of an atom attracting electrons.

74
Q

Electronegativity Trend

A

Greatest in top right; least in bottom left.

75
Q

Ionization Energy

A

Energy required to remove an electron.

76
Q

Ionization Energy Trend

A

Greatest in top right; least in bottom left.

77
Q

Metals Properties

A

Malleable, ductile, conductive, solid at room temperature.

78
Q

Nonmetals Properties

A

Gases or soft solids; poor conductors of heat.

79
Q

Metalloids Properties

A

Brittle, semi-conductive; mix of metal and nonmetal traits.

80
Q

Alkali Metals

A

Group 1, very reactive, one valence electron.

81
Q

Alkaline Earth Metals

A

Group 2, very reactive, two valence electrons.

82
Q

Halogens

A

Group 17, very reactive, seven valence electrons.

83
Q

Noble Gases

A

Group 18, unreactive, eight valence electrons.

84
Q

Transition Metals

A

Groups 3-12, variable valence electrons for bonding.

85
Q

Group vs. Period

A

Groups are vertical; periods are horizontal.

86
Q

Periodic Table Definition

A

Organized elements based on recurring properties.

chemistry (4 decks)

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