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General Chemistry > Quiz 2 (chapter 2-3) > Flashcards

Quiz 2 (chapter 2-3) Flashcards

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1
Q

atom definition

A

the smallest identifiable unit of an element (invisible in greek)

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2
Q

atoms are the key to?

A

connecting the macroscopic and microscopic worlds

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3
Q

how many natural occurring and synthetic elements

A

91 natural
over 20 synthetic

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4
Q

3 most important laws

A

law of conservation mass
law of definite proportions
law of multiple proportions

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5
Q

Dalton’s?

A

atomic theory

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6
Q

J.J. Thomson?

A

discovery of the electron with cathode ray experiment —> Thomson’s atomic model

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7
Q

Milikan?

A

the charge of the electron with oil drop experiment

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8
Q

Rutherford?

A

atomic model with gold foil experiment

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9
Q

J.J Thomson conclusion?

A

the charge-to-mass ratio for the negatively charged electron ( -1.76 x 10^8 C/g)

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10
Q

C?

A

Coloumb (unit for charge)

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11
Q

u?

A

amu (atomic mass unit)

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12
Q

Milikan conclusion?

A

the charge of the electron to be ( -1.60 x 10^-19 C)

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13
Q

How do we deduce the mass of an electron?

A

with the charge of the electron and the mass-to-charge ratio

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14
Q

Rutherford proposed the nuclear theory of the atom, what is part 1?

A

1) most of the atoms mass & all of its positive charge are contained in a small core called NUCLEUS

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14
Q

Rutherford proposed the nuclear theory of the atom, what is part 2?

A

2) most of the volume of the atom is empty space, with tiny, negatively charged ELECTRONS dispersed

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15
Q

Rutherford proposed the nuclear theory of the atom, what is part 3?

A

3) there are as many negatively charged ELECTRONS outside the nucleus as there positively charged PROTONS within the nucleus —> electrically neutral

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16
Q

Rutherford’s model’s flaw?

A

James Chadwick demonstrated that the previously unaccounted for mass was the NEUTRONS (neutral particles in the nucleus)

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17
Q

Mass & charge of neutron

A

mass= similar to proton
charge= no electrical charge

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18
Q

Compare mass of Helium atom with Hydrogen atom

A

Helium is 4 times as massive as Hydrogen —> CAUSE it contains 2 protons & 2 neutrons

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19
Q

atoms are composed with which subatomic particles?

A

protons, neutrons, electrons
*** with nearly identical masses

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20
Q

number of protons defines?

A

the element
***most important number to identify

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20
Q

atomic number?

A

number of protons (which is =number of electrons) in the atom’s nucleus (Z)

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21
Q

***54 elements

A
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22
Q

each element is identified by:

A

a unique atomic number with a unique chemical symbol

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23
Q

isotopes definition

A

atoms with the same # of protons but different # of neutrons (each with a slightly different mass)

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24
Q

mass number definition?

A

the sum of the number of neutrons and protons in an atom (only whole numbers) (A)

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25
Q

mass number equation?

A

A= # protons (p+) + # neutrons (n)
n= A - Z

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26
Q

chemical symbol?

A

element (X)

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27
Q

Isotope notation #1

A

A X
Z

(20 Ne )
(10 )

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28
Q

Isotope notation #2

A

X-A
(Ne-20)

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29
Q

Natural Abundance definition

A

relative amount of each different isotope in a naturally occurring sample of a given element is roughly constant (%)

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30
Q

% abundance equation

A

% abundance Ne-20 = X / (X + Y + Z) x100

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31
Q

ions definition

A

of electrons in a neutral atom = # of protons in its nucleus
***in chemical change, atoms can lose/gain electrons and become charged with particles (IONS)

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32
Q

cations?

A

positively charged ions (Na+)

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33
Q

anions?

A

negatively charged ions

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34
Q

equation to show for ions (gain and loss)

A

Mg —> Mg^2+ + 2e^-
#e- 12 10
#p+ 12 12

     N + 3e^- ---> N^2- #e-   7                     10 #p+  7                      7
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35
Q

Mendeleev’s periodic law

A

when the elements are arranged in order of increasing mass, similar properties recurred in a periodically

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36
Q

Modern periodic table order?

A

increasing atomic number rather than increasing relative mass

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36
Q

Modern periodic table contains?

A

more elements than Mendeleev’s table

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37
Q

***metal, metalloids, nonmetal

A
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38
Q

metals (L) common properties (6)

A

-good conductors of heat & electricity
-malleable (pounded into sheets)
-ductility (drawn into wires)
-often shiny
-lose electron
-form cation

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39
Q

metals exceptions (3)

A

-NOT Hydrogen
-all solid EXCEPT Mercury (liquid)
-including Al & Po

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40
Q

metalloids common properties (3)

A

-also called semimetals
-MIXED properties
-some are semiconductors

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41
Q

metalloids exceptions (1)

A

-NOT Al & Po

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42
Q

nonmetals (R) common properties (6)

A

-poor conductors of heat & electricity
-not malleable
-not ductile
-often shiny
-gain electron
-form anion

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43
Q

nonmetals exceptions (4)

A

-Including Hydrogen
-5 solids (C, P, S, Se, I)
-1 liquid (Br)
-11 gases

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44
Q

main-group elements?

A

properties tend to be predictable based on their position (not the middle ones)

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45
Q

transition elements?

A

properties tend to be less predictable based on their position (middle)

46
Q

noble gas? (3)

A

-group 8A
-also called gas inert
-unreactive

47
Q

alkali metals? (2)

A

-group 1A
-very reactive (create heat; in water)

48
Q

alkaline metals? (2)

A

-group 2A
-fairly reactive

49
Q

halogens? (3)

A

-group 7A
-very reactive nonmetals
-found in nature as a salt (ionic compound)

50
Q

halogens phases? (4)

A

-F (gas)
-Cl (gas)
-Br (liquid)
-I (solid)

51
Q

main-group metals tend to ?

A

lose electrons (forming a cation with same # electrons as nearest noble gas)

52
Q

main-group nonmetals tend to ?

A

gain electrons (forming an anion with same # electrons as nearest noble gas)

53
Q

alkali metals tend to? (1A)

A

lose 1 electron & form 1+ ions

54
Q

alkaline metals tend to? (2A)

A

lose 2 electron & form 2+ ions

55
Q

aluminum tends to? (3A)

A

lose 3 electron & form 3+ ions

56
Q

halogens tend to? (7A)

A

gain 1 electron & form 1- ions

57
Q

oxygen family nonmetals tend to? (6A)

A

gain 2 electron & form 2- ions

58
Q

nitrogen tends to? (5A)

A

gain 3 electron & form 3- ions

59
Q

atomic mass is also called

A

atomic weight or standard atomic weight

60
Q

atomic mass represents?

A

the average mass of the isotopes that compose that element (weighted according to the natural abundance of each isotope)

61
Q

atomic mass equation

A

Atomic mass (Σ) = (fraction isotope 1 x mass) + (fraction isotope 2 x mass)
***fraction isotope= % abundance

62
Q

Mass spectrometer graph (3)

A

-amount of peaks= how many isotopes exist
-x-axis= accurate mass of each isotope in amu
-% abundance= X(height) / (X + Y) x 100

63
Q

how to know the number of atoms?

A

weighing them

64
Q

mole definition

A

the measure of the material containing 6.02214076 x 10^23 particles (1 mol=6.02214076 x 10^23 particles)

65
Q

mole = value of atoms in ?

A

X grams (12 grams of C-12)

66
Q

conversion factor of mol atoms –> atoms

A

1 mol atoms / 6.02214076 x 10^23 atoms

67
Q

molar mass definition

A

the mass of 1 mol of atoms of an element
molar mass (g/mol) = atomic mass units (amu)

68
Q

method to count # of atoms (3)

A

1) mass of element
2) convert into moles
3) convert into atoms (Avogadro)

69
Q

mixture vs compound

A

mixture= elements can mix in any proportions whatsoever (H2, O2)
compound= elements combine in fixed, definite proportions (H2O, fixed amount of H and O)

70
Q

compounds are composed of?

A

atoms held together by CHEMICAL BONDS

71
Q

chemical bonds definition

A

result from the attractions between the charged particles (e- & p+) that compose the atoms

72
Q

two types of chemical bonds?

A

ionic bonds and covalent bonds

73
Q

1) ionic bonds definition

A

-bonds that occur between metals & nonmetals
-transfer of electrons from the metal atom & the nonmetal atom (cation & anion)

74
Q

what happens to metal and nonmetal in an ionic bond?

A

-metal becomes a cation
-nonmetal becomes an anion

75
Q

how an ionic bond forms?

A

the oppositely charged ions attract one another by electrostatic forces

76
Q

in SOLID phases, ionic compound is composed of?

A

a lattice

76
Q

crystal lattice (lattice)

A

3D array of alternating cations & anions

77
Q

2) covalent bonds definition

A

-bonds that occur between 2 or more nonmetals
-transfer of electrons, composing a molecule

78
Q

covalent bonds synonym

A

molecular compounds

79
Q

compound’s chemical formula indicates?

A

-the elements present in the compound
-the relative number of atoms/ions of each

80
Q

3 types of chemical formulas

A

1) empirical formulas
2) molecular formulas
3) structural formulas

81
Q

1) empirical formula?

A

gives the relative number of atoms of each element in a compound (divide by the greatest common factor) (H2O2 –> HO)

82
Q

2) molecular formula?

A

gives the actual number of atoms in each element in the molecule of compound (as it is)

83
Q

3) structural formula?
check pictures

A

-uses lines to represent covalent bonds
-shows how atoms in a molecule are connected/bonded to each other
(H–O–O–H)

84
Q

which chemical formula communicates the most information?

A

structural formula

85
Q

which chemical formula communicates the most information?

A

empirical formula

86
Q

molecular model indicates?

A

a more accurate & complete way to specify a compound

87
Q

4) ball-and-stick molecular model?

A

atoms as balls & chemical bonds as sticks (how the two connect reflects a molecule’s shape)

87
Q

5) space-filling molecular model?

A

atoms fill the space between each other to more closely represent a best estimate of how a molecule will appear if visible

88
Q

molecular type of chemical formulas?

A

molecular models:
4) ball-and-stick model
5) space-filling model

88
Q

elements can be?

A

atomic OR molecular

89
Q

compounds can be?

A

ionic OR molecular

90
Q

atomic elements?

A

exist in nature with single atoms as their basic unit
(all the noble gases & metals)

91
Q

molecular elements?

A

do not exist in nature with single atoms, they exist as MOLECULES (2+ atoms of the element bonded together)

92
Q

molecular element: diatomic elements? (7)

A

H2, N2, O2, F2, Cl2, Br2, I2

93
Q

molecular element: polyatomic elements? (3)

A

P4, S8, Se8

94
Q

molecular compounds are composed of?

A

2 or more covalently bonded nonmetals

95
Q

basic units of molecular compounds?

A

molecules

96
Q

ionic compounds are composed of?

A

cations (usually metal) & anions (usually nonmetal) bound together by ionic bonds (NaCl)

97
Q

basic unis of ionic compounds?

A

formula unit

98
Q

ions can be?

A

monoatomic ions OR polyatomic ions

99
Q

polyatomic ions?

A

composed of a group of covalently bonded atoms with an overall charge

100
Q

ionic compound formulas? (3)

A

1) always contain positive & negative ions
2) sum of cations = sum of anions
3) smaller whole-number ratio (simplify)

101
Q

2 types of ionic compounds?

A

type 1: metal forms only 1 type of ion
type 2: metal forms many types of ion

102
Q

Naming type 1 ionic compounds

A

**metal ion always have the same charge
name of cation + base name of anion (+ide)
(metal) (nonmetal)

103
Q

***know metal ion charges & certain nonmetal

A
104
Q

Naming type 2 ionic compounds

A

**metal can form 2+ kind of cation (must be specified/deduced)
name of cation (charge) + base name of anion (+ide)
(metal) (Roman numerals) (nonmetal)

105
Q

***know metal ion charges that have diff charges

A
106
Q

***charge of type 2 metals= determined by calculations

A
107
Q

***Naming polyatomic ions

A
108
Q

Oxyanions?

A

(most polyatomic ions are oxyanions)
=anions containing oxygen & another element

109
Q

oxyanions= more oxygen atoms VS fewer

A

more oxygen= -ate (nitrate)
fewer oxygen= -ite (nitrite)

110
Q

oxyanions= more than 2 oxygen VS less than 2

A

more than 2 oxygen= per- (perchlorate)
less than 2 oxygen= hypo- (hypochlorite)

111
Q

hydrates?

A

ionic compounds containing a specific number of water molecules associated with each formula unit (x H2O)

112
Q

***hydrate prefixes

A

General Chemistry (2 decks)

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