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Pre-Pharm > Chemistry - Ch 2 > Flashcards

Chemistry - Ch 2 Flashcards

0
Q

Law of constant composition

A

In a given compound, the relative numbers and kinds of atoms are constant

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1
Q

Atoms

A

Smallest particles of an element that retain the chemical identity of the element

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2
Q

Law of conservation of mass/matter

A

Total mass of materials present after a chemical reaction is the same as the total mass present b4 the reaction; basis for Postulate 3

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3
Q

Law of multiple proportions

A

If two elements A & B combine to form more than one compound, the masses of B can combine with a given mass of A are in the ratio of small whole numbers

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4
Q

Subatomic particles

A

Smaller parts of an atom

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5
Q

Cathode rays

A

Radiation originating from the negative electrode (cathode)

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6
Q

Coulomb

A

SI unit for electrical charge

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7
Q

Charge of a single electron

A

1.602 x 10^-19

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8
Q

Thomson’s charge to mass ratio

A

1.76 x 10^8 C/g

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9
Q

Mass of electron

A

9.10938 x 10^-28g; 2000 times smaller than hydrogen (lightest atom)

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10
Q

Radioactivity

A

Spontaneous emission of radiation; discovered by Henri Becquerel, who urged Marie Curie & her husband Pierre to isolate the radioactive components of uranium

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11
Q

3 types of radiation

A

Ernest Rutherford: alpha , beta, gamma (y); each type responds differently in an electric field - a & b are bent by it; y is unaffected

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12
Q

Beta rays

A

High speed electrons; = radioactive element of cathode rays; attracted to a positively charged plate

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13
Q

Alpha rays

A

Positive charge; attracted toward a negative plate

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14
Q

Gamma rays

A

High energy radiation similar to x-rays; does not consist of particles, carries no charge

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15
Q

Nucleus

A

Mass of atom & all of its positive charge reside in this very small dense region per Ernest Rutherford in his scattering experiment, which disproved JJ Thomson’s plum pudding model; protons & neutrons reside in nucleus

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16
Q

Discovery of protons (+ particles)

A

1919, Ernest Rutherford

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17
Q

Discovery of neutrons (neutral)

A

1932, James Chadwick

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18
Q

Proton charge (electronic charge)

A

+1.602 x 10^-19 C

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19
Q

Every atom has ___________ number of electrons & protons so atoms have no net electrical charge

A

Equal

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20
Q

1 Atomic mass unit (amu)

A

1.66054 x 10^-24g; protons & neutrons’ masses nearly equal, both much greater than an electron; proton’s mass: 1.0073 amu; neutron: 1.0087 amu; electron: 5.486 x 10^-4 amu; 1g= 6.02214 x 10^23amu

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21
Q

Angstrom

A

Non SI unit of length to express atomic dimensions

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22
Q

Atomic number

A

Number of protons in the nucleus of an atom

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23
Q

Mass number

A

Element symbol with subscript & superscript to left; superscript = mass # (protons + neutrons); subscript = atomic # (# of protons or electrons)

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24
Q

Isotopes

A

Atoms with identical atomic numbers but different mass numbers(same # of protons, different # of neutrons)

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25
Q

Average atomic mass

A

Masses of its various isotopes & their relative abundances

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26
Q

Mass spectrometer

A

Most direct and accurate means for determining atomic & molecular weights

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27
Q

Mass spectrum

A

Graph of the intensity of the detector signal vs particle atomic mass

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28
Q

Periodic table

A

Most significant tool chemists use for organizing & remembering chemical facts; arrangement of elements in order of increasing atomic number, with elements having similar properties placed in vertical columns

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29
Q

Periods

A

Horizontal rows of periodic table

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30
Q

Groups

A

Vertical columns of periodic table; AB designations with Arabic or Roman numerals, or IUPAC (Internat’l union of pure chemistry) 1-18 with no letters; similar properties b/c same arrangement of electrons @ periphery of their atoms

31
Q

Coinage metals

A

Copper (cu), silver (ag), & gold (au); pt of gp 1B

32
Q

Alkali metals (1A)

A

Li, Na, K, Rb, Cs, Fr

33
Q

Alkaline earth metals (2A)

A

Be, Mg, Ca, Sr, Ba, Ra

34
Q

Chalcogens (6A)

A

O, S, Se, Te, Po

35
Q

Halogens (7A)

A

F, Cl, Br, I, At

36
Q

Noble/rare gases (8A)

A

He, Ne, Ar, Kr, Xe, Rn

37
Q

Metallic elements (metals)

A

All elements on left side and in middle of periodic table except hydrogen; share properties - luster, high electrical/heat conductivity; solid @ rm temp (except mercury)

38
Q

Nonmetallic elements (nonmetals)

A

Separated from metals on table by diagonal steplike line from boron (B) to astatine (At); includes hydrogen; @ rm temp, some gaseous, some solid, 1 liquid; differ from metals in appearance & other physical properties

39
Q

Metalloids

A

Elements that lie along line between metals & nonmetals that have properties that fall btwn both (ex.antimony-Sb)

40
Q

Nuclear reactions

A

Reaction btwn uranium & neutrons that creates plutonium

41
Q

Transuranium elements

A

Elements beyond uranium (92) on periodic table; not found in nature; can only be synthesized via nuclear reactions

42
Q

Molecule

A

Assembly of 2+ atoms tightly bound together

43
Q

Chemical formula

A

Represents molecular form of an element

44
Q

Diatomic molecule

A

Molecule made up of 2 atoms; hydrogen (H2), oxygen (O2), nitrogen (N2) & the halogens (F2, Cl2, Br2, I2) normally occur as diatomic molecules

45
Q

Ozone

A

O3; sharp, pungent smell, toxic

46
Q

Molecular compounds

A

Compounds composed of molecules (contain more than 1 type of atom)

47
Q

Molecular formulas

A

Chemical formulas that indicate actual numbers and types of atoms in a molecule

48
Q

Empirical formulas

A

Chemical formulas that only give the relative number of atoms of each type of molecule; subscripts = smallest possible whole # ratios

49
Q

Structural formula

A

Shows which atoms are attached to which within the molecule; atoms represented by chemical symbols, lines represent bonds

50
Q

Perspective drawing

A

Drawing a structural formula to show the angles at which atoms are joined together

51
Q

Ball-and-stick model

A

Show atoms as spheres & bonds as sticks; accurately represents angles of attachment

52
Q

Space-filling model

A

Depicts what the molecule would look like if the atoms were scaled up in size; angles hard to see

53
Q

Ion

A

Charged particle formed by removing or adding electrons to a neutral atom; positively charged ion = cation; negatively charged ion = anion

54
Q

Metal ions _______ electrons to form cations; nonmetals ________ electrons to form anions

A

Lose;gain

55
Q

Polyatomic ions

A

Atoms joined as a molecule but with a net positive or negative charge (ex. NH4+, ammonium ion; or SO4 2-, sulfate ion)

56
Q

Ionic compound

A

Compound with both positively & negatively charged ions; in general cations are metal ions & anions are nonmetal ions; ionic compounds are generally combos of metals & nonmetals ex. NaCl (molecular compounds generally = nonmetals only ex.H2O); only empirical formulas can be written for most ionic compounds

57
Q

Chemical nomenclature

A

System used in naming substances (Latin nomen - name - & calare - to call)

58
Q

Organic compounds

A

Carbon, usually in combo with hydrogen, oxygen, nitrogen, or sulfur; all other compounds are inorganic

59
Q

Monatomic ions

A

Ions formed from a single atom

60
Q

Transition metals

A

Metals that can form more than one cation; occur in middle block of elements on periodic table, from group 3B to 2B; 1A (Na+, K+, & Rb+), 2A (Mg2+, Ca2+, Sr2+, Ba2+), 3A (Al3+) & 2 transition metal ions Ag+ (1B) & Zn2+ (2B) form only 1cation

61
Q

Cations formed from nonmetal ions have names that end in _________

A

-ium ex. NH+4 (ammonium ion); H3O+ (hydronium ion); both ex are polyatomic; vast majority of cations are monatomic metal ions

62
Q

Monatomic anions (neg ions) are formed by replacing ending with ______

A

IDE ex H- (hydride); O2- (oxide); N3- (nitride); a few simple polyatomic anions have names ending in IDE (OH- = hydroxide; CN- = cyanide; O2 2- = peroxide)

63
Q

Oxyanions

A

Polyatomic anions containing oxygen; end in -ate (most common oxyanion of an element) or -ite (oxyanion that has same charge but 1 atom fewer (ex. NO3- = nitrate; NO2- = nitrite)

64
Q

Anions derived by adding H+ to an oxyanion are named by adding as a prefix the word ____ or _____

A

Hydrogen or dihydrogen (ex. CO3 2- : carbonate ion; HCO3- : hydrogen carbonate; PO4 3- : phosphate ion; H2PO4 - : dihydrogen phosphate ion; each H+ reduces the negative charge of the parent ion by 1; older method for naming is to use prefix bi- (HCO3- = bicarbonate)

65
Q

Prefix hypo

A

One O atom fewer than oxyanion ending in ite ex. ClO2- = chlorite; ClO- = hypochlorite (one O atom fewer than chlorite)

66
Q

Ionic compounds consist of the ____name followed by the ____ name

A

Cation; anion (ex. CaCl2 = calcium chloride)

67
Q

Acid

A

substance whose molecules yield hydrogen (h+) ions when dissolved in water; composed of an anion connected to enough H+ ions to neutralize/balance the anion’s charge

68
Q

Acids containing anions whose names end in -ate or -ite or named by changing -ate to ___ and -ite to ___ then adding the word acid

A

-ic; -ous (Ex. ClO4 - : perchloric –> HClO4 (perchloric acid); ClO3 - : chlorate –> HClO3 (chloric acid); ClO2- : chlorite –> HClO2 (chlorous acid); ClO- : hypochlorite –> HClO (hypochlorous acid)

69
Q

Names & Formulas of Binary Molecular Compounds - 3 Rules

A

(1) Name of element farther to left in table usually written 1st (exception = Oxygen; always last except when combined with fluorine (2) if both elements are in the same group, the one having the higher atomic # is named 1st (3) name of 2nd element is given an -ide ending (4) Greek prefixes are used to indicate # of atoms of each element; mono never used with 1st element; prefix ends in a or o & the name of 2nd begins with a vowel, a or o is often dropped

70
Q

Prefixes for Naming Binary Compounds (10)

A

Mono (1), Di (2), Tri (3), Tetra (4), Penta (5), Hexa (6), Hepta (7), Octa (8), Nona (9), Deca (10)

71
Q

Organic Chemistry

A

study of compounds of carbon

72
Q

Hydrocarbons

A

Compounds that contain only carbon and hydrogen

73
Q

Alkanes

A

each carbon atom is bonded to four other atoms (3 simplest = methane, CH4 =1 carbon; ethane, C2H6 = 2 carbons, & propane, C3H8 = 3 carbons); 4C = butane; 8 = octane (C8H18)

74
Q

Functional groups

A

specific groups of atoms

75
Q

Alcohol

A

Obtained by replacing an H atom of an alkane with an -OH group; replace -ane ending with -ol

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