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chem spring exam (pt. 2) Flashcards

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1
Q

summarize the connection between Coulomb’s law and period trends

A

an increased atomic number means there’s an increased number of protons, with an increased number of protons then the strength of positive nuclear charge increases, and then with that the attraction force on electrons increases

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2
Q

what does Coulomb’s law explain about periodic trends?

A

it explains why we see the trends we do in atomic radii, reactivity, electronegativity, and others

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3
Q

increases going down and increases when moving left in a period

A

atomic radius

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4
Q

metals increase going down and moving left in a period

A

metal reactivity

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5
Q

nonmetals increase going up and moving right in a period

A

nonmetal reactivity

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6
Q

increases when going UP a group and when moving RIGHT in a period

A

electronegativity

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7
Q

increases when going up a group and when moving right in a period (not electronegativity)

A

ionization energy

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8
Q

atoms that lose electrons become ______

A

smaller

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9
Q

atoms that gain electrons become _____

A

larger

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10
Q

increases as you move DOWN a group

A

atomic radius

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11
Q

how does shielding effect work?

A

electrons in the inner energy levels block the attraction of the nucleus to the valence electrons, and thus they become more loosely held

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12
Q

increases as you move DOWN a group because the atomic size is increasing

A

shielding effect

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13
Q

what bond forms when the EN is larger than 2

A

ionic bond

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14
Q

what bond forms when the EN is less than 0.5?

A

covalent bond

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15
Q

what bond forms when the EN is between 0.5 and 2?

A

polar covalent bond

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16
Q

what happens to electrons in an ionic bond?

A

they are transferred from one to another

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17
Q

what happens to electrons in a covalent bond?

A

they are equally shared between the two

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18
Q

what happens to electrons in a polar covalent bond?

A

they are unequally shared

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19
Q

list the oxidation numbers for groups 1 and 2, and for 13-17

A
  1. +1
  2. +2
  3. +3
  4. +/- 4
  5. -3
  6. -2
  7. -1
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20
Q

which of the following elements has the largest atomic radius?

a.) Cr
b.) Ca
c.) Ba
d.) Cs

A

Cs

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21
Q

which of the following metals has the highest reactivity?

a.)Ba
b.) Ru
c.) W
d.) Mg

A

Ba

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22
Q

which of the following nonmetal has the lowest reactivity?

a.) Xe
b.) F
c.) C
d.) Kr

A

Xe

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23
Q

which of the following has the highest shielding effect?

a.) Pd
b.) C
c.) Bi
d.) Fr

A

Fr

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24
Q

which of the following has the highest electronegativity?

a.) Kr
b.) Zr
c.) C
d.) Mg

A

C

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25
which of the following has the highest ionization energy? a.) F b.) Zn c.) Be d.) Fr
F
26
what do electrons do in an ionic bond?
transfer
27
what type of elements make up an ionic bond?
metal and nonmetal
28
what type of boiling point does an ionic bond have?
high
29
t/f? ionic bonds CAN conduct electricity when dissolved in water?
true
30
LiF, Pb(SO4), and NaCl are examples of what type of bond?
ionic
31
what do electrons do in a covalent bond?
share
32
what type of elements make up a covalent bond?
two nonmetals
33
what type of melting/boiling point do covalent bonds have?
low
34
t/f? covalent bonds CANNOT conduct electricity when dissolved in water?
true
35
H20, P(Cl3), and NH3 are all examples of what type of bond?
covalent
36
what do the electrons do in a metallic bond?
delocalized e- create a "sea of e-"
37
what elements are involved in a metallic bond?
metals only
38
what states of matter can be had with metallic bonds?
solid and liquid
39
what is the type of boiling/melting point of a metallic bond?
varies
40
what are two properties of a metallic bond?
good conductors of heat good conductors of electricity
41
Fe. Au, Ag, Lu, and Al are all _____
malleable
42
Pt, Au, and Lu are all ____
ductile
43
Au and Ag are both ____
luster
44
rose gold, bronze, brass, sterling silver, and carbon steel are all examples of _____
an alloy
45
how do you determine the bond of 2 elements?
subtract the two EN of each element thus determining the type of bond
46
intermolecular forces are _____ different substances
between
47
intramolecular forces are _____ the same substance
within
48
what is meant by the statement "bonding is a spectrum"?
there aren't just two types of bonds. it's a spectrum with ionic and nonpolar at the two extremes
49
write a sentence to summarize the connections between chemical bonds, chemical reactions, and compounds
chemical bonds from through chemical reactions and form new compounds
50
explain why most atoms from chemical bonds and why noble gases do not
they form bonds to become stable with a full outer energy level of e- noble gases don't form chemical bonds because they are already stable
51
explain the difference between what a chemical formula tells you about an ionic vs. a covalent compound
a covalent compound- the chemical formula tells you exactly the number and types of atoms ionic- represents the ratio of cations to anions in the crystal lattice
52
ionic bonds are always between ____
ions
53
ionic bonds can result in the formation of a what?
salt
54
covalent compounds result in the formation of a what?
molecule
55
which bond is a crystalline solid?
ionic
56
which bond can be any state of matter?
covalent
57
list the number of atoms in each element in the compound below: Ca(ClO3)2
calcium - 1 chlorine - 2 oxygen - 6
58
explain the connection between EN and the formation of an ionic bond
the difference in EN is so great that one atom takes the e- from the other because it has such a greater attraction to them
59
use an example of an ionic compound to explain the rule of "zero charge"
MgCl2 - magnesium has a +2 charge and there are two Cl atoms, each having a charge of -1 these cancel each others charges out
60
explain why it's necessary to include a Roman numeral when naming an ionic compound with a transition metal
you can't determine the charge of a transition metal from the periodic table, so the Roman numeral indicates the charge of the metal ion
61
give an example of a common compound and how the properties of the compound differ from those of the elements by themselves
NaCl is table salt we can eat Na is explosive with water Cl is poisonous alone
62
name the following compounds: (NH4)(C2H3O2) Mn(OH)2
ammonium acetate manganese (II) hydroxide
63
write the chemical formula for the following: Calcium phosphate Lead (IV) sulfate
Ca3(PO4)2 Pb(SO4)2
64
describe the unique properties that result from metallic bonds
malleable ductile can conduct electrical and thermal energy strong absorbers and reflectors of light
65
explain the connection b/w EN and the formation of a covalent bond
when the EN difference is small, and not big enough for one atom to take the e- from the other, the atoms are shared instead in a covalent bond
66
2 shared e-
single bond
67
4 shared e-
double bond
68
6 shared e-
triple bond
69
name the following compounds (with numbers) SO2 B2H4
sulfur dioxide diboron tetrahydride
70
write the chemical formula for the following: diphosphorus trisulfide boron tribromide
P2S3 BBr3
71
do not impact a substance's identity
physical change (states of matter can change)
72
result in a new substances from a chemical reactions occurring
chemical change
73
boiling, melting, vaporizing, and grinding are all examples of what
physical change
74
burning, oxidizing, rotting, fermenting are all examples of what
chemical change
75
reacting particles must collide with enough energy for a chemical reaction to occur
collision theory
76
how can you tell that a chemical reaction has occurred?
release of light release of heat sudden color change odor change gas released formation of a precipitate
77
matter cannot be created nor destroyed in a system, it can only change forms
law of conservation of mass
78
how does the law of conservation of mass relate to chemical reactions?
the mass of the reactants must be equal the mass of the products
79
2 or more reactants combine to form a new compound
synthesis
80
1 reactant breaks down into 2 or more products
decomposition
81
when a substance reacts (burns) with O2
combustion
82
1 element replaces a like element in a compound
single
83
when ions in 2 compounds swap and make 2 new compounds
double

Junior (20 decks)

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