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zGeneral Chemistry 1 > Unit 2-Atoms, Molecules, and Ions > Flashcards

Unit 2-Atoms, Molecules, and Ions Flashcards

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1
Q

Dalton’s Atomic Theory

A
  1. Matter is composed of atoms
  2. An element is composed entirely of ONE TYPE of atom
  3. A compound contains atoms of 2 or more different elements. The rel # of atoms of each element in a compound is always the same
  4. Atoms do not change identity in chem reactions; only the ways in which they are joined change
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2
Q

Atoms

A

the smallest units of an element that have all the properties of that element

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3
Q

The Law of Constant Composition

A

all samples of a PURE substance contain the same elements in the same proportion by mass

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4
Q

Law of Multiple Proportions

A

when the same elements from more than one compound, the mass of 1 element that combines with a fixed mass of a second element are in a ratio of small whole #s

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5
Q

Law of Conservation of Mass

A

there is No detectable change in mass when a chem reaction occurs

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6
Q

Rutherford’s conclusions
(study notes on experiment)

A
  • a nucleus that is very small compared to the atom, has a high pos charge and contains most of the mass of the atom
  • the remainder space is mostly empty and has electrons
  • proton in nucleus, pos charged with equal magn to neg charge of electron (equal # of protons and electrons)
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7
Q

atomic # (z) =

A

of protons

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8
Q

mass # (A) =

A

sum of protons and neutrons

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9
Q

isotopes

A

atoms of an element whose nuclei contain diff #s of neutrons (same atomic #, diff mass #)
Symbol: A/z X

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10
Q

Ions

A

charged particles created from a atom gaining/losing e-
Charge= P+ - e-

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11
Q

cation

A

pos charge from losing e-

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12
Q

anion

A

neg charge from gaining e-

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13
Q

atomic mass

A

1/12 mass of one 12C atom
(atomic mass=mass #u)

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14
Q

mass spectrometer

A

used to measure the masses and abundance of isotopes

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15
Q

isotopic mass

A

mass (a) of a particular isotope

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16
Q

atomic mass

A

the weighted avg mass of the naturally occurring isotopes of the element
(atomic mass = decimal %(A)isotopic mass(A) + decimal %(B)isotopic mass(B) + …)

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17
Q

periodic table

A

arranges the elements with similar properties in same column

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18
Q

period

A

a horizontal row (inc #)

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19
Q

group (family)

A

vertical column containing chem similar elements (properties)

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20
Q

metal

A
  • element that’s shiny and is a good electrical conductor.
  • center and left side of table
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21
Q

nonmetal

A
  • typically a nonconductor
  • top right of table
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22
Q

metalloid

A
  • has properties of both metals and nonmetals
  • staircase sep metals and nonmetals
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23
Q

representative element

A

the elements in the A groups (1, 2, 13-18)

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24
Q

transition metals

A

elements in the B groups (3-12)

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25
Q

inner-transitional metals

A

2 rows of metals (Ianthanides and actinides) set at bottom of table

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26
Q

alkali metals

A

soft, reactive metals in 1A

27
Q

alkaline earth metals

A

elements in groups 2A

28
Q

Halogens (aka salt-formers)

A

reactive NONMETALS in group 7A (17)

29
Q

Noble gases

A

the stable, largely inert gases in group 8A (18)

30
Q

molecules

A

a combination of atoms joined so strongly that they behave as a single particle

31
Q

diatomic

A

contains 2 atoms

32
Q

homonuclear diatomic

A

contain 2 of same atoms (N2)

33
Q

heteronuclear diatomic

A

contain 2 different atoms (NO)

34
Q

elements

A

all atoms in molec are same (O2)

35
Q

molec compounds

A

2 or more elements form a molec (H2O)
- typicalyl from nonmetals

36
Q

molec formula

A

gives # of every type of atom in molec

37
Q

structural formula

A

shows how the atoms are connected in molec

38
Q

molecular mass

A

sum of atomic masses of all atoms present in the molec formula expressed in atomic mass units (u)

39
Q

ionic compounds

A

composed of cations and anions forming a neutral species
- usually metal + nonmetal
- cation surrounded by anion or vice versa

40
Q

empirical formula

A

uses the smallest whole # subscription to express the relative # of ions
- rel # of ions balance charges to zero

41
Q

polyatomic ions

A

a group of atoms with a net charge that behaves as a single particle

42
Q

formula mass of ionic compounds

A

the sum of the atomic masses of all atoms in the empirical formula of an ionic compound

43
Q

chemical nomenclature

A

the organized system for naming compounds

44
Q

naming ionic compounds

A
  • cation then anion
    monoatomic ions:
  • cation same
  • anion = name + “ide”
45
Q

naming transition metals

A

for metals that form 1+ cation, a roman numeral = charge of ion is shown in parenthesis following name of element

46
Q

acids

A

a compound that produces hydrogen cations when dissolved in water

47
Q

naming acids

A

anions ending in:
- “ide” are changed to “ic” and prefix “hydro” added along with “acid”
- “ate” are changed to “ic” and “acid” added
- “ite” are changed to “ous” and “acid” added

48
Q

naming of molec (nonmetal) compounds

A

first element followed by second ending in “ide”

49
Q

order of element names

A
  1. elements farther to left of table is first
  2. elements closer to bottom w/in group is first
  3. hydrogen is first when combined w/ 6A and 2A element; is second when combined w/ 1A-5A
  4. oxygen is second; except with flourine
50
Q

numerical prefixes in molecular compound names

A

some elements form 1+ compound. Add numerical prefixes (mono-, di-, tri-, tetra-, penta-, hexa-) (mono usually omitted for first element).
- Ex: CO = carbon monoxide

51
Q

hydrocarbons

A

organic compounds that contain only the elements hydrogen and carbon

52
Q

alkanes

A

hydrocarbons with formula CnH2n+2

53
Q

cycloalkanes

A

hydrocarbons with a ring of carbon atoms and formula CnH2n

54
Q

functional groups

A

atoms or small groups of atoms that undergo characteristic reactions
- Alcohols = -OH
- Ethers= C-O-C

55
Q

Alkane nomenclature

A
  • suffix -ane with proper prefix (# carbon atoms):
    one = meth-
    two = eth-
    three = prop-
    four = but-
    fix = pent-
    six = hex-
    (ex: CH4 = methane)
56
Q

Cycloalkane nomenclature

A

alkane nomenclature + prefix “cyclo”
(Ex: cyclopropane)

57
Q

substituent: alkyl group

A

alkane with one hydrocarbon removed
- base alkane name w/ “-yl” ending

58
Q

substituent: halides

A

add “oro” ending

59
Q

Properties of ionic compounds

A
  • metals and nonmetals
  • hard, brittle solids
  • high melting point
60
Q

Properties of molecular compounds

A
  • metals
  • some liquid/gas at room temperature
  • low melting point
61
Q

dissociation of ionic compounds

A

ionic compounds dissociate into individual cations and anions when dissolved in water

62
Q

electolytes

A

a substance that forms ions in water solution
- conduct electricity

63
Q

nonelectolytes

A

water and compounds that dissolve in water as neutral molecules
- do not conduct electricity
- MOST molecular compounds

zGeneral Chemistry 1 (13 decks)

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