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AP Chem > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Who were the first to try to explain why chemical changes occur and described matter?

A

Greeks

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2
Q

Who discovered several elements & learned to prepare the mineral acids?

A

Alchemists

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3
Q

Who created the foundations of modern chemistry in 1400s-1500s?

A

Georg Baur; Paracelsus

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4
Q

First chemist to perform truly quantitative experiments

A

Robert Boyle

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5
Q

Who said “phlogiston” flows out of burning material? Who discovered oxygen gas?

A

Stahl; Joseph Priestley

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6
Q

Who explained nature of combustion & carefully weighed reactants & products?

A

Antoine Lavoisier

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7
Q

Define law of conservation of mass

A

Mass is neither created nor destroyed

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8
Q

Lavoisier showed combustion involved __ & life is supported by it

A

Oxygen

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9
Q

Who found that copper carbonate is always 5.3 parts Cu, 4 parts O, 1 part C by mass?

A

Joseph Proust

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10
Q

Define law of definite proportion

A

A given compound always contains exactly the same proportion of elements by mass

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11
Q

Dalton said if elements have ___, compounds always have the __ __ of atoms

A

Particles; Same combination

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12
Q

Define law of multiple proportions

A

When 2 elements form a series of compounds, the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to small whole numbers

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13
Q

Describe Dalton’s theory (4)

A

1) each element is made up of tiny particles called atoms 2) atoms of a given element are identical; the atoms of different elements are different in some way3) chemical compounds are formed when atoms of different elements combine with each other; a given compound always has the same relative numbers & types of atoms4) chemical reactions involve reorganization of the atoms- changes in the way they are bound together; the atoms are not changed in a chemical reaction

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14
Q

Define atomic mass (atomic weights)

A

The weighted average mass of the atoms in a naturally occurring element

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15
Q

Who developed the modern symbols for elements used in writing formulas?

A

Berzelius

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16
Q

Describe Avogadro’s hypothesis

A

At the same temperature & pressure, equal volumes of different gases contain the same number of particles

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17
Q

1860: who found the correct atomic mass of carbon is 12?

A

Cannizzaro

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18
Q

Describe JJ Thompson’s experiments

A

Studied electrical discharges in cathode-ray tubes; found when high voltage was applied to the tube, a cathode ray was produced; ray was a stream of electrons

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19
Q

Define cathode rays

A

Ray emanating from the negative electrode (cathode) in a partially evacuated tube; a stream of electrons

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20
Q

What did Thompson postulate about the atom?

A

An atom consists of a diffuse cloud of positive charge with negative electrons embedded randomly in it, which created the plum pudding model of the atom

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21
Q

Define electrons

A

Negatively charged particle that moves around the nucleus of an atom

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22
Q

Define radioactivity

A

The spontaneous decomposition of a nucleus to form a different nucleus

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23
Q

Three types of radioactive emission

A

Gamma rays; Beta particles; Alpha particles

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24
Q

Define gamma ray; Define beta particle; Define alpha particle

A

High-energy “light”; High-speed electron; 2+ charge

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25
Q

Define nucleus

A

Small, dense center of positive charge in an atom

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26
Q

What did Rutherford discover?

A

Metal-foil experiment: shot alpha particles at thin foil, some particles deflected (caused by a center of concentrated positive charge containing most of the mass

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27
Q

Define nuclear atom

A

Atom with a dense center of positive charge with electrons moving around the nucleus at a distance that is large relative to the nuclear radius

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28
Q

Mass of electron; Mass of proton & neutron

A

9.11 • 10^-31 kg; 1.67 • 10^-27 kg

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29
Q

Define proton

A

Positively charged particle in an atomic nucleus

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30
Q

Define neutron

A

Particle in the nucleus with the same mass as a proton with no charge

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31
Q

The nucleus is almost all of an atom’s __; electrons constitute most of the atomic __

A

Mass; Volume

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32
Q

__ affect interactions with other atoms; atoms of different __ have different chemical behavior; number of __ must equal number of __ to have no net charge

A

Electrons; Elements; Electrons; Protons

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33
Q

Define isotope

A

Atom with the same number of protons but different number of neutrons

34
Q

Define atomic number

A

Number of protons in the nucleus of an atom

35
Q

Define mass number

A

Total number of protons and neutrons in the nucleus of an atom

36
Q

Isotopes show almost identical __ properties

A

Chemical

37
Q

Nucleus size; Atom size; Charge of electron/proton

A

10^-13 cm; 10^_8 cm; 1.60 • 10^-19 C

38
Q

Define covalent bond

A

A type of bond in which electrons are shared by atoms

39
Q

Define chemical bond

A

The force, or more accurately, the energy, that holds two atoms together in a compound

40
Q

Define molecule

A

A bonded collection of 2 or more atoms of the same or different elements

41
Q

Define structural formula

A

The representation of a molecule in which the relative positions of the atoms are shown and the bonds are indicated by lines

42
Q

Define chemical formula

A

The representation of a molecule in which the symbols for the elements are used to indicate the types of atoms present and subscripts are used to show the relative numbers of atoms

43
Q

Define Ball-and-stick model

A

A molecular model that distorts the sizes of atoms but shows bond relationships clearly

44
Q

In a compound composed of molecules, the individual molecules move around __

A

Independently

45
Q

Define space-filling model

A

A model of a molecule showing the relative sizes of the atoms and their relative orientations

46
Q

Define cation

A

A positive ion; formed by loss of an electron

47
Q

Define ion

A

An atom or a group of atoms that has a net positive or negative charge

48
Q

Define anion

A

A negative ion; formed by gain of an electron

49
Q

Define ionic bonding

A

The electrostatic attraction between oppositely charged ions

50
Q

Define ionic solid (salt)

A

A solid containing cations & anions that dissolves in water to give a solution containing the separated ions which are mobile and this free to conduct electricity (simple or polyatomic ions)

51
Q

Define polyatomic ion

A

An ion containing a number of atoms

52
Q

Define metals

A

An element that gives up electrons relatively easily to form positive ions & is lustrous, malleable, ductile, & a good conductor of heat and electricity

53
Q

Define periodic table

A

A chart showing all the elements arranged in columns with similar chemical properties

54
Q

Define malleable; Define ductility

A

Can be hammered into thin sheets; Can be pulled into wires

55
Q

Define nonmetals

A

An element not exhibiting metallic characteristics; chemically, typical nonmetals accept electrons from a metal to form negative ions

56
Q

Define transition metals

A

Metals shown in the center of the periodic table

57
Q

Nonmetals often bond __ with __ and reacts with __ to form __

A

Covalently; Nonmetals; Metals; Salts

58
Q

Define groups (families)

A

A vertical column of elements having the same valence electron configuration and showing similar chemical properties

59
Q

Define alkali metals

A

Group 1A metals; very active elements that readily form ions with a 1+ charge when they react with nonmetals

60
Q

Define alkaline earth metals

A

Group 2A metals; all form ions with a 2+ charge with nonmetals

61
Q

Define halogens

A

Group 7A elements; all form diatomic molecules and react with metals to form salts containing ions with a 1- charge

62
Q

Define noble gases

A

Group 8A elements; all exist under normal conditions as monatomic (single-atom) gases and have little chemical reactivity

63
Q

Define Periods

A

Horizontal rows of elements in the periodic table

64
Q

Define binary compounds

A

Compounds composed of 2 elements

65
Q

To name binary ionic compounds: (3)

A

1) cation is always named first, then the atom2) monatomic cations have the same name as its parent element 3) monatomic anions are named by taking the root of the element name and adding -ide

66
Q

Define binary ionic compound

A

Contains a positive ion (cation) and a negative ion (anion)

67
Q

In formulas of ionic compounds, simple ions are represented by the __ __

A

Element symbol

68
Q

The __ on the metal ion must be specified when a metal can form more than one type of positive ion; __ __ indicate the charge of the cation

A

ChargeRoman numerals

69
Q

The ion with the higher charge has a name ending in __, and the one with the lower charge has a name ending in __

A

-ic; -ous

70
Q

Elements that form only one cation don’t need to be identified by a __ __

A

Roman numeral

71
Q

A compound must be __ __; compounds containing __ __ usually having a Roman numeral in its name

A

Electrically neutral; Transition metals

72
Q

Although __ & __ are transition metals, they are usually named without a Roman numeral because in virtually all of its compounds, it is found as the __ & __ ions

A

Silver; Zinc; Ag+; Zn+2

73
Q

When a metal ion is present that forms more than one type of cation, the charge on the metal ion must be determined by __ the __ & __ charges of the compound

A

Balancing; Positive; Negative

74
Q

Define oxyanion

A

Anions that contain an atom of a given element and different #s of oxygen atoms

75
Q

When there are 2 members in a series, the one with the smaller # of oxygen atoms ends in __, and the name of the one with the larger # ends in __

A

-ite; -ate

76
Q

When more than 2 oxyanions make up a series, __ (less than) and __ (more than) are used as prefixes to name the members of the series with the fewest & the most oxygen atoms

A

Hypo-; Per-

77
Q

__ __ __ element names follow the same rules as binary ionic compounds

A

Binary covalent compounds

78
Q

Define binary covalent compounds

A

Compounds formed between two nonmetals

79
Q

To name binary covalent compounds: (4)

A

1) the first element in the formula is named first using the full element name2) the second element is named as if it were an anion 3) prefixes are used to denote the number of atoms present 4) the prefix mono- is never used for naming the first element

80
Q

The final _ or _ of the prefix is usually dropped when the element starts with a vowel

A

O; A

81
Q

Define acid

A

A substance that produces hydrogen ions in solution; a proton donor (can be viewed as a molecule with one or more H+ ions attached to an anion

82
Q

To name acids (4)

A

1) if the anion does not contain oxygen, the acid is named with the prefix hydro- and the suffix -ic2) if the anion contains oxygen, the acidic name is formed from the root name of the anion with a suffix of -ic or -ous, depending on the name of the anion3) if the anion name ends in -ate, the suffix -ic is added to the root name 4) if the anion name ends in -ite, the -ite is replaced by -ous

AP Chem (11 decks)

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