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Chemistry 1004 > Unit 1 Intro & Measurement > Flashcards

Unit 1 Intro & Measurement Flashcards

1
Q

Describe the solid state of matter

A

-definite volume
-maintains shape regardless of container
-particles are close together and in a regular pattern
-high density

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2
Q

Describe the liquid state of matter

A

-definite volume
-takes shape of its container
-particles are close together and move past each other -difficult to compress

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3
Q

Describe the gas state of matter

A

-no definite shape
-assumes shape of container
-no definite volume
-particles are far apart and move around randomly

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4
Q

Describe the plasma state of matter

A

-highly charged particles
-high kinetic energy
-no fixed shape or volume
-less dense than solids or liquids
-ions roam freely

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5
Q

What is a mixture?

A

-composed of more than 1 component
-varying composition
-any combo of solid, liquid, or gas
-can be separated into its components by physical process

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6
Q

Examples of mixtures

A

-sugar dissolved in water
-salt water
-air (mix of gases)
-solutions, colloids, suspensions

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7
Q

What are the 2 types of mixtures & describe them

A

-heterogeneous mixture = visually distinguishable components (salt & pepper, oil & water)

-homogeneous mixture = appear uniform throughout, all solutions are homogenous not all homogenous mixtures are solutions (milk: uniform appearance, but still has fat particles floating around)

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8
Q

What is matter?

A

anything that has mass / takes up volume

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9
Q

What 2 categories can matter be divided into based on its PHYSICAL changes ?

A

pure substances & mixtures

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10
Q

What is a pure substance?

A

-composed of only a single component (atom or molecule)
-has a consistent composition
-cannot be broken down into other pure substances by a physical change
-either an element or a compound

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11
Q

How is a pure substance different from a mixture?

A

-mixtures are composed of more than one component
-mixtures have varying composition
-mixtures can be separated into their components by physical process

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12
Q

What is an element?

A

a pure substance that cannot be broken down by a chemical change

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13
Q

What is a compound?

A

a pure substance formed by chemically joining two or more elements chemical combo of 2 or more elements (salt = NaCl, water H2O)

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14
Q

What two things can be separated by CHEMICAL means?

A

compounds & molecules

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15
Q

What is an atom?

A

the building blocks of all matter

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16
Q

What is a molecule

A

-a group of atoms bonded together
-the smallest unit of a chemical compound that can take part in a chemical reaction
-elements contain molecules, compounds are molecules of that compound

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17
Q

What are diatomic molecules?

A

molecules that contain 2 atoms that are chemically bonded

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18
Q

What are the 7 naturally occurring diatomic molecules?

A

-Hydrogen (gas)
-Nitrogen (gas)
-Fluorine (gas)
-Oxygen (gas)
-Iodine (solid)
-Chlorine (gas)
-Bromine (liquid)

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19
Q

What are physical properties?

A

things that can be measured without changing the composition of the sample under study

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20
Q

Examples of physical properties

A

-mass
-color
-volume
-density
-solubility
-odor
-melting point / boiling point

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21
Q

What are chemical properties

A

chemical reactions / changes

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22
Q

Examples of chemical properties

A

-flammability
-toxicity
-heat of combustion
-pH value
-rate of radioactive decay
-chemical stability

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23
Q

What are the signs that a chemical change occurs?

A

-color change
-formation of precipitate
-formation of gas
-odor change
-temperature change
-production of light
-volume change
-change in taste or smell
-formation of bubbles

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24
Q

“mega” prefix meaning

A

10^6

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25
Q

“kilo” prefix meaning

A

10^3

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26
Q

“deci” prefix meaning

A

10^-1

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27
Q

“centi” prefix meaning

A

10^-2

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28
Q

“milli” prefix meaning

A

10^-3

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29
Q

“micro” prefix meaning

A

10^-6

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30
Q

“nano” prefix meaning

A

10^-9

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31
Q

What are the building block elements of the human body (96%)

A

-oxygen
-carbon
-hydrogen
-nitrogen

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32
Q

What are the 3 subatomic particles that atoms are composed of?

A

-protons
-neutrons
-electrons

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33
Q

Describe the nucleus

A

-location of protons and neutrons
-dense core of the atom
-location of most of the atom’s mass

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34
Q

Describe the electron cloud

A

-location of electrons
-comprises most of the atom’s volume
-mostly empty space

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35
Q

Atomic number is equal to what?

A

the number of protons in the nucleus

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36
Q

What are isotopes?

A

atoms of the same element that have different #s of neutrons same atomic number, different mass number

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37
Q

What are principal energy levels / shells (n)?

A

the region around the nucleus that is occupied by electrons with particular energy

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38
Q

Which electrons are closer to the nucleus?

A

electrons in the lower numbered shells

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39
Q

Which electrons are further from the nucleus?

A

electrons in higher numbered shells

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40
Q

What are the subshells labeled as & how many orbitals do they each have?

A
  • s = 1 orbital
  • p = 3 orbitals
  • d = 5 orbitals
  • f = 7 orbitals
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41
Q

How many electrons can each orbital hold?

A

2

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42
Q

What are orbitals?

A

region of space where the probability of finding an electron is high

43
Q

List the properties of metals

A

-located on the left side & middle of the periodic table
-good conductors of heat and electricity
-malleable (thin sheets)
-ductile (thin vials)
-shiny solids at room temperature (except mercury (Hg) which is a liquid)

44
Q

List the properties of nonmetals

A

-located on the right side of the periodic table
-have a dull appearance
-usually poor conductors of heat & electricity
-can be solids, liquids or gases at room temp

45
Q

List the properties of metalloids/semi-metals

A

-located on the solid line that starts at boron (B) and angles down towards astatine (At)
-have properties intermediate between metals and nonmetals
-**only 7 metals are metalloids: boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), & astatine (At)

46
Q

What is specific gravity?

A

-a quantity that compares the density of a substance with the density of water at the same temperature

47
Q

What is the density of water?

A

1g/mL

48
Q

How many elements are there?

A

117

49
Q

Major minerals:

A

elements that are needed (at least 100mg daily)
-magnesium & sulfur

50
Q

Mass number =

A

number of protons + number of neutrons

51
Q

of neutrons =

A

atomic mass - atomic number

52
Q

H

A

hydrogen

53
Q

He

A

helium (noble gas)

54
Q

Li

A

lithium (alkali metal)

55
Q

Be

A

beryllium (alkaline earth metal)

56
Q

B

A

boron (metalloid)

57
Q

C

A

carbon (non-metal)

58
Q

N

A

nitrogen (non-metal)

59
Q

O

A

oxygen (non-metal)

60
Q

F

A

fluorine (halogen)

61
Q

Ne

A

neon (noble gas)

62
Q

Na

A

sodium (alkali metal)

63
Q

Mg

A

magnesium (alkaline earth metal)

64
Q

Al

A

aluminium (metal)

65
Q

Si

A

silicon (metalloid)

66
Q

P

A

phosphorous (non-metal)

67
Q

S

A

sulfur (non-metal)

68
Q

Cl

A

chlorine (halogen)

69
Q

Ar

A

argon (noble gas)

70
Q

K

A

potassium (alkali metal)

71
Q

Ca

A

calcium (alkaline earth metal)

72
Q

Sc

A

scandium (transitional metal)

73
Q

Ti

A

titanium (transitional metal)

74
Q

Mn

A

manganese (transitional metal)

75
Q

Fe

A

iron (transitional metal)

76
Q

Co

A

cobalt (transitional metal)

77
Q

Ni

A

nickel (transitional metal)

78
Q

Cu

A

copper (transitional metal)

79
Q

Ge

A

germanium (metalloid)

80
Q

As

A

arsenic (metalloid)

81
Q

Br

A

bromine (halogen)

82
Q

Kr

A

krypton (noble gas)

83
Q

Ag

A

silver (transitional metal)

84
Q

Sb

A

antimony (metalloid)

85
Q

Te

A

tellurium (metalloid)

86
Q

I

A

iodine (halogen)

87
Q

Au

A

gold (transitional metal)

88
Q

Hg

A

mercury (transitional metal)

89
Q

Pb

A

lead (metal)

90
Q

What is atomic weight?

A

the weighted average of all the masses of the naturally occurring isotopes of a particular element (located below the chemical symbol)

91
Q

What is the unit for atomic weight?

A

amu (atomic mass units)

92
Q

how do you calculate amu?

A

(fraction (%) of 1 isotope x mass of isotope 1) + (fraction of isotope 2 x mass of isotope 2)…

93
Q

what is natural abundance?

A

the amount the particular isotope/element is naturally occurring

94
Q

isotopic abundance needs to be:

A

in decimal form

95
Q

halogens

A

-only exist as two atoms together (diatomic)
-very reactive

96
Q

noble gases

A

-very stable
-rarely reactive with other elements

97
Q

alkali metals & alkaline earth metals

A

-soft* shiny metals
-good conductors of heat and electricity

98
Q

what is the formula for calculating how many electrons each shell can hold ?

A

2n^2

99
Q

What are valence electrons?

A

Valence shell = the outermost shell (highest value of n), the electrons in that shell are valence electrons

100
Q

What is the Lewis structure?

A

electron-dot structure , it represents the valence electrons of a particular element

101
Q

Why does atomic size increase as we go down a group on the periodic table?

A

Because the number of shells increases

102
Q

Why does atomic size decrease as we go left to right on the periodic table?

A

the number of electrons is increasing, therefore attracting more energy and shrinking its size

103
Q

What is ionization energy?

A

the energy needed to remove an electron from a neutral atom

104
Q

Why does ionization energy decrease as we go down the periodic table?

A

valence electrons get farther away from the positively charged nucleus

Chemistry 1004 (4 decks)

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