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chemistry > Untitled Deck > Flashcards

Untitled Deck Flashcards

(86 cards)

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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
aufbau principle
each electron occupies the lowest energy orbital allowed
26
metalloids
combo for both metals and metals-they can be both conductors and nonconductors
27
periodic law
the properties of elements vary periodically with their atomic numbers
28
sublevel (energy)
contained by principal energy levels
29
group
boxes arranged in order by similar traits
30
valence electrons
electrons in the atom's outermost orbitals
31
Pauli (exclusion) principle
a maximum of z electrons can occupy a single atomic orbital but with opposite spins
32
periods
boxes arranged in order by similar number of protons electrons
33
Representative elements
the elements in groups 1,2, and 13-18 process a wide range of chemical and physical groups.
34
John Newlands contribution to the periodic table
arranged elements by increasing atomic mass
35
Dmitri Mendeleev contribution to the periodic table
found a connection between atomic mass and properties, and predicted the existence and properties of undiscovered elements
36
Henry Mosely contribution to the periodic table
he arranged the periodic table based on atomic number
37
Aufbau Principle
the lowest level must be filled before moving up
38
Pauli Exclusion Principle
If two electrons occupy the same orbital, they must have opposite spins.
39
Hund's Rule
Electrons will fill an orbital one at a time before pairing up to have the same
40
What is the difference between an orbital, energy level, and sublevel?
An energy level is the largest category that defines the periods of the periodic table.
41
Within the energy level there are various sublevels. Some sublevels have multiple orbitals.
42
What is electronegativity?
how likely an atom is to attract electrons, making it negative. (Electro-negative)
43
How are elements in a group similar and what is the cause of their similarity?
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
What are the typical properties of metals?
- shiny
45
-Malleable
46
-Good conductor
47
-Solid at room temperature
48
-give away electrons more easily
49
What are the typical properties of nonmetals?
-take electrons more easily
50
-gases or soft
51
-Brittle
52
-not good conductors
53
What are the general properties of metalloids?
-mix of metals and nonmetals
54
-Shiny but brittle
55
-semiconductors.
56
Alkali metals
Group 1 elements except for hydrogen, very very reactive, have one valence electron
57
Alkaline earth metals
Group 2 elements, very reactive, have 2 valence electrons
58
Halogens
Group 17, very very reactive, have 7 valence electrons
59
Noble gases
Group 18, very unreactive, have 8 valence electrons
60
Transition metals
groups 3-12, variable valence electrons
61
John Newlands
Arranged elements by atomic mass; rule of octaves.
62
Dmitri Mendeleev
Predicted undiscovered elements based on atomic mass.
63
Henry Mosely
Established atomic number; resolved periodic table issues.
64
Valence Electrons Group 2
Elements in group 2 have 2 valence electrons.
65
Valence Electrons Group 17
Elements in group 17 have 7 valence electrons.
66
Aufbau Principle
Electrons fill lower energy orbitals first.
67
Pauli Exclusion Principle
Electrons in same orbital must have opposite spins.
68
Hund's Rule
Electrons occupy orbitals singly before pairing.
69
Energy Level
Largest category defining periodic table periods.
70
Sublevel
Divisions within energy levels containing orbitals.
71
Atomic Radius
Measurement of space occupied by electron cloud.
72
Atomic Radius Trend
Decreases across a period; increases down a group.
73
Electronegativity
Likelihood of an atom attracting electrons.
74
Electronegativity Trend
Greatest in top right; least in bottom left.
75
Ionization Energy
Energy required to remove an electron.
76
Ionization Energy Trend
Greatest in top right; least in bottom left.
77
Metals Properties
Malleable, ductile, conductive, solid at room temperature.
78
Nonmetals Properties
Gases or soft solids; poor conductors of heat.
79
Metalloids Properties
Brittle, semi-conductive; mix of metal and nonmetal traits.
80
Alkali Metals
Group 1, very reactive, one valence electron.
81
Alkaline Earth Metals
Group 2, very reactive, two valence electrons.
82
Halogens
Group 17, very reactive, seven valence electrons.
83
Noble Gases
Group 18, unreactive, eight valence electrons.
84
Transition Metals
Groups 3-12, variable valence electrons for bonding.
85
Group vs. Period
Groups are vertical; periods are horizontal.
86
Periodic Table Definition
Organized elements based on recurring properties.

chemistry (4 decks)

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