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CHEM 119 > Unit 1: Matter > Flashcards

Unit 1: Matter Flashcards

1
Q

define matter

A

anything that has mass and volume

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2
Q

define pure substances

A

matter that is uniform throughout and cannot be separated by physical means

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3
Q

define mixture

A

two or more pure substances physically combined

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4
Q

examples of mixtures

A
  • koolaid
  • air
  • steel (alloy, solid mixture)
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5
Q

define heterogenous mixture

A

a mixture that is NOT the same throughout (ex: salad)

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6
Q

define homogenous mixture

A
  • aka solution
  • a mixture that is the same throughout (ex: koolaid)
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7
Q

define elements

A

a pure substance consisting of a single type of atom

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8
Q

define compounds

A

a pure substance that is the chemical combination of two or more elements (ex: NaCl, salt)

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9
Q

what are the two types of pure substances

A
  • elements
  • compounds
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10
Q

what is the difference between salt water and NaCl salt

A
  • salt water can be separated by physical means, is a mixture
  • NaCl salt is a pure substance and must be separated by chemical means
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11
Q

what is the simplest alcohol

A

methanol

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12
Q

is natural water containing ions and compounds a mixture or pure substance

A
  • mixture
  • homogenous (solution)
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13
Q

is distilled/deionized water a mixture or pure substance

A
  • pure substance
  • contains only water molecules and is uniform throughout
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14
Q

describe the 3 types of matter

A
  • solid: organized, rigid
  • liquid: moving, close particles
  • gas: independent particles
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15
Q

describe the volume and shape of the 3 types of matter

A
  • solid: definite volume and shape
  • liquid: definite volume, indefinite shape
  • gas: indefinite volume and shape
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16
Q

define physical properties

A

can be measured or observed without changing the composition or identity of the substance

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17
Q

examples of physical properties

A
  • density
  • conductivity
  • melting point
  • color
  • hardness
  • temperature
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18
Q

define chemical properties

A

describe the way a substance may change or react to form other substances

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19
Q

examples of chemical properties

A
  • flammability
  • corrosivity
  • reactivity
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20
Q

define chemical reactions

A

occur during chemical changes

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21
Q

what is the gas in the bubbles of pure water boiling

A
  • water (H2O)
  • boiling is a phase change (physical) so the water will stay the same substance
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22
Q

define extensive properties

A

properties that depend on the amount of matter present (scalar)

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23
Q

examples of extensive properties

A
  • mass
  • volume
  • surface area
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24
Q

define intensive properties

A

properties that do not depend on the amount of matter present

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25
Q

examples of intensive properties

A
  • melting point
  • density
  • temperature
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26
Q

what is the mass and charge of protons, neutrons, and electrons

A
  • protons: 1amu, 1+
  • neutrons: 1amu, 0
  • electrons: 1 amu, 1-
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27
Q

what distinguishes elements from each other

A

number of protons

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28
Q

how do neutral atoms become ions

A

gaining or losing electrons

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29
Q

define cations

A
  • positive charge
  • more protons
  • usually formed by metals
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30
Q

define anions

A
  • negative charge
  • more electrons
  • usually formed by nonmetals
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31
Q

how was an amu previously defined

A

1/12 of the weight of a 12C atom

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32
Q

define isotopes

A

atoms with the same number of protons (atomic number) and different number of neutrons (mass number)

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33
Q

what is used to determine the existence of different isotopes and how does it work

A
  • mass spectrometry
  • ionized isotopes are separated based on the difference in mass
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34
Q

what is the atomic mass

A

mass of the average of all the isotopes

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35
Q

how do you find atomic mass when given the weight and abundance of isotopes

A
  • weighted average
  • (% abd of 1st isotope as decimal)(mass of 1st isotope) + (% abd of 2nd isotope as decimal)(mass of 2nd isotope)
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36
Q

what is the most abundant isotope in natural uranium

37
Q

what uranium isotope is needed to use in nuclear power plants

38
Q

what % U-235 is needed for reactor grade uranium

39
Q

what % U-235 is needed for weapons grade uranium

40
Q

how is uranium enrichment accomplished

A
  • centrifuge
  • heavier isotopes move to the edge and the lighter isotope can be extracted
41
Q

define periodic table

A

systemic catalog of elements arranged in order of atomic number

42
Q

what are the rows and columns of a periodic table called

A
  • rows: periods
  • columns: groups
43
Q

what is the name of group 1 in the periodic table

A

alkali metals

44
Q

what is the name of group 2 in the periodic table

A

alkaline earth metals

45
Q

what is the name of group 6 in the periodic table

A

chalcogens

46
Q

what is the name of group 7 in the periodic table

47
Q

what is the name of group 8 in the periodic table

A

noble gases

48
Q

define chemical compounds

A

formed from fixed ratios of atoms or ions

49
Q

define ionic compounds

A
  • usually formed between cations (metals) and anions (nonmetals)
  • can also be formed between polyatomic ions
50
Q

define covalent

A
  • formed between nonmental atoms
51
Q

define empirical formula

A
  • simplest whole number ratio of atoms of each element in a compound
  • always used for ionic compounds
52
Q

define molecular formula

A
  • exact number of atoms of each element in an individual molecule
  • covalent compounds have molecular formulas
53
Q

define structural formula

A

drawing of the connectivity of the atoms

54
Q

example of the empirical and molecular formula for hydrogen peroxide

A
  • empirical: HO
  • molecular: H2O2
55
Q

how are ionic compounds formed

A

metal transfers electrons to a nonmetal

56
Q

what is the charge of elements in groups 1, 2, 6, 7

A
  • 1: 1+
  • 2: 2+
  • 6: 2-
  • 7: 1-
57
Q

what is the charge of Al, Zn, Cd, Ag

A
  • Al: 3+
  • Zn: 2+
  • Cd: 2+
  • Ag: 1+
58
Q

describe the naming system of oxyanions in the group halogens (number of oxygens and prefixes)

A
  • know the number of oxygens in the -ate form
  • one less oxygen in the -ite form
  • two less oxygens in the hypo-ite form
  • one more oxygen in the per-ate form
  • hypo-ite to ite to ate to per-ate
59
Q

what order do you write ionic compounds in

A
  • metal cation first
  • nonmetal anion second
60
Q

describe how you write the formula for ionic compounds

A
  • metal cation first and nonmetal anion second
  • make the charges equal by adding subscripts (ex: +2=-2)
  • make sure subscripts are in empirical formula
61
Q

describe how to name an ionic compound

A
  • write metal cation first
  • write nonmetal anion: if element change ending to -ide, if polyatomic ion write its name
62
Q

what must you include in the name of a compound where the cation can have more than one possible charge

A
  • write roman numeral of charge in parenthesis
  • ex: iron(III) nitrate
63
Q

define molecule

A

aggregate of at least two atoms held together by covalent bonds

64
Q

define covalent bonds

A

electrons are shared between nonmetal atoms

65
Q

what formula should you write covalent compounds in

A

molecular or structural formulas

66
Q

define diatomic elements and list them

A
  • elements that naturally occur as molecules containing two atoms (O with subscript 2)
  • H2, N2, O2, F2, Cl2, Br2, I2
67
Q

define acid

A
  • covalent
  • contains H+ and an anion
  • give off H+ in water
68
Q

define inorganic compounds

A
  • covalent
  • contains nonmetals
69
Q

define organic compounds

A
  • covalent
  • contains C and H (sometimes O)
70
Q

how do you know the amount of H+ to have in an acid

A

H+ must balance with the charge of the anion

71
Q

acids must have balanced charges so does this mean they are ionic compounds

A
  • no
  • acids are covalent not ionic
72
Q

explain how to name acids

A
  • anion ends with -ide: hydro_ic acid (HF, hydrofluoric acid)
  • anion ends with -ate: _ic acid (HNO3, nitric acid)
  • anion ends with -ite: _ous acid (HNO2, nitrous acid)
73
Q

explain how to name binary covalent compounds

A
  • prefix used to denote number of atoms of each element in the compound
  • don’t use mono- for first element
74
Q

what 3 things does the mass number of an element represent

A
  • average weight of a single atom in amu
  • average weight of one mole of atoms in grams
  • average weight of 6.022E23 atoms in grams
75
Q

define avogadro’s number

A
  • 6.02E23
  • number of atoms in 1 mole
76
Q

how many moles of oxygen are in 1 mole of glucose, C6H12O6

77
Q

how do you find the molar mass of a molecule

A

multiply the number of atoms of each element by its atomic mass and add them all together

78
Q

what measurement is needed to figure out how many moles of glucose are in 10g

A
  • molar mass of glucose
  • 180.12g = 1 mole glucose
79
Q

define solution

A
  • homogenous mixture of two or more substances
  • can be liquid, solid, or gaseous
80
Q

define solvent

A

substance present in the greatest quantity in a solution

81
Q

define solute

A
  • substances other than the solvent in a solution
  • solutes are dissolved in the solvent
82
Q

define aqueous solution

A

liquid solution in which the solvent is water

83
Q

define concentration

A

amount of solute present in a given quantity of solvent or solution

84
Q

define molarity

A
  • molar concentration
    moles of solute per liter of solution
85
Q

explain solution preparation

A
  • measure the amount of solute you want
  • funnel solute into volumetric flask
  • add a portion of the solvent to the flask
  • swirl the mixture until all of the solute is dissolved
  • add additional solvent needed
86
Q

why shouldn’t you pour all of the solvent into the solute when creating a solution

A
  • the solute will take up volume as it is dissolved in the solvent
  • for precise measurements of a solution you must wait for the solute to dissolve and take up volume before adding the rest of the solvent
87
Q

define dilution

A

procedure for preparing a less concentrated solution from a more concentrated (stock) solution

88
Q

what is the equation for dilution

A
  • M1V1 = M2V2
  • molarity of concentrated times volume of concentrated = molarity of diluted time volume of diluted

CHEM 119 (8 decks)

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