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Principles of Chemistry (Lecture) > Module 4: Nomenclature > Flashcards

Module 4: Nomenclature Flashcards

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1
Q

This is an abbreviation used to indicate an element or an atom of an element

A

Chemical symbols

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2
Q

Atoms of the same element that differ in mass

A

Isotopes

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3
Q

who discovered isotopes?

A

Fredrick Soddy

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4
Q

What is different from isotopes of the same element?

A

Number of neutrons

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5
Q

isotope of Hydrogen with no neutron

A

Protium

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6
Q

isotope of Hydrogen with one neutron

A

Deuterium

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7
Q

isotope of Hydrogen with two neutron

A

Tritium

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8
Q

This is approximately equal to the mass number of an element

A

Atomic mass

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9
Q

A weighted, average mass of all the isotopes present in a naturally occurring sample of that element

A

Atomic Mass

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10
Q

Atomic mass is expressed in?

A

atomic mass unit (amu)

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11
Q

Formula for average atomic mass unit

A

Summation of fraction abundance of one isotope x isotopic mass and so on

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12
Q

The instrument used to experimentally determine the occurrence and natural abundances of isotopes

A

Mass Spectrometry

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13
Q

An electrically charged atom

A

Ion

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14
Q

all ions are atoms?

A

True

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15
Q

all atoms are ions?

A

False

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16
Q

an atom that gains one or more electrons

A

Anion

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17
Q

a negatively charged ion

A

Anion

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18
Q

an atom that loses one or more electrons

A

Cation

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19
Q

a positively charged ion

A

Cation

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20
Q

Name for Group 1 in the periodic table

A

Alkali metals

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21
Q

Name for Group 2 in the periodic table

A

Alkaline earth metals

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22
Q

Name for Group 15 in the periodic table

A

Pnictogens

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23
Q

Name for Group 16 in the periodic table

A

Chalcogens

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24
Q

Name for Group 17 in the periodic table

A

Halogens

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25
Q

Name for Group 18 in the periodic table

A

Noble Gases

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26
Q

It is the representation of a molecule with the use of chemical symbols to indicate the type of atoms with a subscript that indicate the number of atoms of each type

A

Molecular Formula

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27
Q

It shows how the atoms are connected in a molecule

A

Structural Formula

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28
Q

It shows the molecular geometry of a molecule

A

Ball and Stick Model

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29
Q

It focus on showing the electron cloud of a molecule

A

Space-filling Model

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30
Q

Electron Cloud

A

areas of higher probability of finding an electron which is always in motion

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31
Q

true chemical formula of a compound

A

Molecular Formula

32
Q

lowest number ratio possible of a compound

A

Empirical Formula

33
Q

Elements that tend to lose electrons to become cations

A

Metals

34
Q

Elements that tend to gain electrons and become anions

A

Non-metals

35
Q

Compound formed when a metal reacts with a nonmetal in which a transfer of electrons between the two occurs which is stabilized by ionic bonds

A

Ionic Compound

36
Q

electrostatic forces of attraction between oppositely charged ions of an ionic compounds

A

Ionic bonds

37
Q

Nomenclature for binary ionic compounds

A

cation first and anion second
change ending of anion to “-ide”
add roman numeral for cations that can have multiple charges

38
Q

Ions composed of more than one atom that act as a discrete unit and are electrically charged molecules

A

Polyatomic ions

39
Q

polyatomic ions containing at least one oxygen

A

Oxyanions

40
Q

Ammonium

A

Nh4 +

41
Q

Peroxide

A

O2 2-

42
Q

Hydroxide

A

OH-

43
Q

Acetate

A

C2H3O2 -

44
Q

Cyanide

A

CN -

45
Q

Carbonate

A

CO3 2-

46
Q

Bicarbonate

A

HCO3 -

47
Q

Nitrate

A

NO3 -

48
Q

Nitrite

A

NO2 -

49
Q

Sulfate

A

SO4 2-

50
Q

Sulfite

A

SO3 2-

51
Q

Hydrogen sulfate

A

HSO4 -

52
Q

Phosphate

A

PO4 3-

53
Q

Hydrogen phosphate

A

HPO4 2-

54
Q

Dihydrogen phosphate

A

H2PO4 -

55
Q

Perchlorate

A

ClO4 -

56
Q

Chlorate

A

ClO3 -

57
Q

Chlorite

A

ClO2 -

58
Q

Hypochlorite

A

ClO -

59
Q

Chromate

A

CrO4 2-

60
Q

Dichromate

A

Cr2O7 2-

61
Q

Permanganate

A

MnO4 -

62
Q

Oxalate

A

C2O4 2-

63
Q

Thiosulfate

A

S2O3 2-

64
Q

Compounds that consist of discrete, neutral molecules that results when atoms share electrons through covalent bonds

A

Molecular Compounds

65
Q

Compounds that often exist as gases, low-boiling liquids and low-melting solids

A

Molecular Compounds

66
Q

Compounds that often exist as solids that have high boiling and melting points

A

Ionic Compounds

67
Q

Compounds that formed between two nonmetals

A

Molecular Compounds

68
Q

Nomenclature for Binary Molecular Compounds

A

more metallic element first and more nonmetallic element second
add numerical prefixes to both elements (except mono in the more metallic element)
Change ending of more nonmetallic element to “-ide”

69
Q

compounds that comprised of hydrogen and one other nonmetallic element in aqueous state

A

Binary Acids

70
Q

Nomenclature for Binary Acids (aq)

A

“hydro-“ prefix
other nonmetallic element with “-ide” suffix
and the word “acid”

71
Q

Nomenclature for Binary Acids (s)

A

the word “hydrogen”

change ending of nonmetallic element to “-ide”

72
Q

Compounds that contain hydrogen, oxygen and at least one other element bonded in a way that it impart acidic properties to the compound

A

Oxyacids

73
Q

Compounds that typically consist of hydrogen combined with a polyatomic ion containing oxygen

A

Oxyacids

74
Q

Nomenclature for Oxyacids

A

No “hydrogen” word
start with root name of anion and replace ending for “-ate” to “-ic” and for “-ite” with “-ous”
add the word “acid”

75
Q

Nomenclature for Oxyacids with more than 2 ternary acids

A

No “hydrogen” word
start with root name of anion and replace ending for highest number of atom, “per-“ and “-ic” ; “-ic” ; “ous” ; “hypo-“ and “-ous” for lowest number of atom
add the word “acid”

Principles of Chemistry (Lecture) (7 decks)

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