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Honors Chemistry 2022-2023 > 53 Elements > Flashcards

53 Elements Flashcards

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1
Q

Hydrogen

A

H

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2
Q

Helium

A

He

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3
Q

Lithium

A

Li

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4
Q

Beryllium

A

Be

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5
Q

Boron

A

B

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6
Q

Carbon

A

C

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7
Q

Nitrogen

A

N

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8
Q

Oxygen

A

O

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9
Q

Fluorine

A

F

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10
Q

Neon

A

Ne

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11
Q

Sodium

A

Na

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12
Q

Magnesium

A

Mg

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13
Q

Aluminium

A

Al

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14
Q

Silicon

A

Si

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15
Q

Phosphorus

A

P

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16
Q

Sulfur

A

S

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17
Q

Chlorine

A

Cl
Argon

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18
Q

Argon

A

Ar

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19
Q

Potassium

A

K

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20
Q

Calcium

A

Ca

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21
Q

Titanium

A

Ti

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22
Q

Chromium

A

Cr

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23
Q

Manganese

A

Mn

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24
Q

Iron

A

Fe

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25
Q

Cobalt

A

Co

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26
Q

Nickel

A

Ni

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27
Q

Copper

A

Cu

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28
Q

Zinc

A

Zn

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29
Q

Gallium

A

Ga

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30
Q

Arsenic

A

As

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31
Q

Selenium

A

Se

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32
Q

Bromine

A

Br

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33
Q

Krypton

A

Kr

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34
Q

Rubidium

A

Rb

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35
Q

Strontium

A

Sr

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36
Q

Palladium

A

Pd

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37
Q

Silver

A

Ag

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38
Q

Cadmium

A

Cd

39
Q

Tin

A

Sn

40
Q

Antimony

A

Sb

41
Q

Tellurium

A

Te

42
Q

Iodine

A

I

43
Q

Xenon

A

Xe

44
Q

Caesium

A

Cs

45
Q

Barium

A

Ba

46
Q

Platinum

A

Pt

47
Q

Gold

A

Au

48
Q

Mercury

A

Hg

49
Q

Lead

A

Pb

50
Q

Bismuth

A

Bi

51
Q

Radon

A

Rn

52
Q

Francium

A

Fr

53
Q

Radium

A

Ra

54
Q

First Theory and is it true or false

A

All matter is made of tiny particles called
atoms; indivisible and indestructible units

False because atoms ARE destructable (Dalton believed that atoms were solid spheres)

55
Q

2nd theory, true or false?

A

All atoms of a given element are identical.
False because number neutrons and electrons can vary

56
Q

Third theory, true or false

A

Atoms of a given element are different from
those of any other element.
True, the number of protons always differs

57
Q

4th Theory, true or false

A

Atoms of one element can combine with
atoms of other elements to form compounds.
True, a given compound always has the same
relative number and type of atoms

58
Q

5th theory, true or false

A

Atoms are neither created nor destroyed in
chemical reactions
True. They are only created or destroyed in nuclear fusion or fission

59
Q

Nuclear Symbol Notation

A

A on top, Z on bottom, X
A=mass number
Z=atomic number
X=element symbol

60
Q

Periodic Table Notation

A

Z above X
Z=Atomic number

61
Q

Hyphen Notation

A

X-A
A= Mass number

62
Q

Properties of metals

A

Lustrous, malleable, ductile, conductive, tend to form cations by losing electrons in reactions with nonmetals

63
Q

Properties of nonmetals

A

Tend to form anions by gaining electrons in reactions with metals, generally lack defining properties as they all vary property-wise but they are bad conductors

64
Q

Law of Conservation of Mass

A

Mass is neither created nor destroyed in chemical reactions (for example: the carbon atom in coal becomes carbon dioxide when it is burned)

65
Q

Group 1

A

Alkali Metals

66
Q

Group 2

A

Alkaline Earth Metals

67
Q

Group 17

A

The Halogens

68
Q

Group 18

A

The Noble Gasses

69
Q

Elements left of the staircase

A

Metals (except for Hydrogen)

70
Q

Elements right of the staircase

A

Nonmetals

71
Q

Elements that border the staircase

A

Metalloids

72
Q

Elements located in groups 3-12

A

Transition metals

73
Q

Elements below the main section fo the periodic table

A

Lanthanides (1st row) and Actinides (2nd row)

74
Q

Down a group, ionization energy

A

Decreases

75
Q

Down a group, atomic radius

A

Increases

76
Q

Across a period, ionization energy

A

Increases

77
Q

Across a period, atomic radius

A

Decreases

78
Q

Ionization energy defintion

A

The amount of energy needed to remove an electron

79
Q

Tallest point of wave

A

Crest

80
Q

Lowest point of wave

A

Trough

81
Q

Height of wave

A

Amplitude

82
Q

Distance from highest point to highest point on wave

A

Wavelength

83
Q

Thomson

A

Plum pudding model (electrons floating in positive cloud) and cathode ray tube (proved that electrons were negatve bc they were attracted to the positively charged end of the tube)

84
Q

Rutherford

A

Discovered positive nucleus through gold foil experiment

85
Q

Isotopes

A

Atoms with the same number of protons but different numbers of neutrons

86
Q

Bohr Model of the Atom

A

Circular orbits (quantized energy levels), electrons moved between the orbits by absorbing or emitting particular photons.

87
Q

Schrodinger’s Wave Mechanical Model

A

Probablity map: 95% chance electron is within shaded region, more electrons in darker regions vs. lighter regions.

88
Q

Principle Energy level

A

Distance between electrons and nucleus

89
Q

Quantized energy levels

A

Variation of energy levels, electrons can only possess certain discrete energy levels

90
Q

Aufbau Principle

A

Electrons fill orbitals in order of increasing energy subshells

91
Q

Pauli exclusion principle

A

No two electrons can have the same spin or be in the same location at the same time; this limits repulsion

92
Q

Hund’s Rule

A

Each orbital must contain one electron before a second electron is paired; limits repulsion

93
Q

number of electrons per energy level formula

A

2(n)^2

Honors Chemistry 2022-2023 (4 decks)

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