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Chem-exam prep Flashcards

1
Q

Mass number is…

A

Number of protons and neutrons of an atomic nucleus

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2
Q

Atomic number is…

A

Number of protons in an atomic nucleus

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3
Q

Isotopes are…

A

Atoms with the same elements and atomic number but different mass number

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4
Q

Mole is a…

A

Counting term- relating to the amount of substance that contains the same number of particles as there are atoms in 12g of 12C

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5
Q

the symbol for mole…

A

n

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6
Q

metallic substances conduct as a…

A

Solid and liquid

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7
Q

Ionic substances conduct as a..

A

Liquid and not as a solid

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8
Q

Covalent substances conduct as a…

A

Neither a solid nor liquid-doesn’t conduct at all-

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9
Q

what is lead…

A

Metallic lattice

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10
Q

what makes a lattice structure?

A

High mtp, regular repeating pattern

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11
Q

what is Na electron configuration

A

1s22s22p63s1

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12
Q

What makes a molecular structure

A

Low melting point, covalently bonded

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13
Q

volatile…

A

How easily something turns into a gas

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14
Q

How to determine is a substance is volatile

A

Low boiling/melting point- always never conducts

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15
Q

non-volatile=

A

High boiling point

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16
Q

Energy is required to…

A

break bonds

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17
Q

Particles held tightly in fixed positions..

A

-are not free to move
-cannot conduct

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18
Q

Hard def…

A

How easy it is for a substance to be scratched

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19
Q

Sea of delocalized electrons…

A

formed by valence electrons through pure metals, therefore becoming a positive ion.

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20
Q

valence=

A

outside shell

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21
Q

metallic lattice…

A

regularly arrangement of positive ions embedded in a sea of delocalized electrons

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22
Q

metallic bond…

A

electrostatic force of attraction between layers

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23
Q

Rigid=

A

won’t bend but will break

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24
Q

Strong bonds have…

A

High melting points

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25
Greater the charge=
stronger the attraction
26
Little particles are more...
Tightly packed together
27
bigger particles are...
loose
28
What makes ionic compounds conduct as a liquid?
=>Ion released from a lattice structure =>free to move =>solution conducts electricity
29
Allotropes=
Different form of the same element
30
what is octet expansion?
Forms more bonds in some cases
31
example of a V -shaped
Water- polar
32
why is something polar
Vector sum of bond gives resultant molecular dipole
33
melting only breaks....bonds
secondary
34
what makes a shape v-shaped
Extra pair of electrons
35
low molar mass, LDFS are....
insignificant
36
High molar mass=
Big LDFS, possibly most significant
37
electrons are constantly moving -jumping from....to...
polar to non-polar
38
LDFS=
Temporary dipole
39
Dipole-Dilpoe interactions=
Permanent dipole
40
H-bonds are way stronger than...
DP-DP interactions
41
Dp-Dp interactions are stronger than..
LDFS
42
N.O.FS are Hydrogen bonds bonded to
Nitrogen, oxygen or fluorine
43
H-bonding is the most significant secondary bonding due the large...of primary bonds involved.
Polarity.
44
N.O.FS have a ....boiling point
high
45
ion-dipole interactions is the....of the secondary bonds
strongest
46
LDFS- are the....secondary bonds
weakest
47
only .... bonds connects NOFS
covalent
48
def of hydro-carbon
compounds made of hydrogen and carbon bonds
49
Viscosity=
how easy it flows
50
Honey has a...viscosity
high
51
Longer chain=.....viscosity
Higher viscosity
52
butane=
4
53
empirical formula=
simplest ratio eg: C4H10=C2H5
54
Alkanes have a lower...
melting point
55
magnetic attracts
Magnetic
56
polar attracts
Polar
57
less polarity effect=
longer carbon chain
58
hex=
six
59
pent=
five
60
hept=
7
61
oct=
8
62
dec=
10
63
prop=
three
64
meth=
1
65
ethe=
2
66
tertiary=
the carbon the hydroxyl is bonded to three other carbon atoms
67
oxidation changes from...to...
from orange to green
68
primary alcohol=alcohol-->aldehyde-->
carboxylic acid
69
secondary alcohol=2 alcohol--->
ketone
70
tertiary alcohol=alcohol--->
does not produce an observable change-difficult to oxidize
71
hydrophobic...
wont dissolve in water
72
hydrophilic=
will dissolve in water
73
what does "VSEPR" stand for
Valence shell electron pair repulsion
74
VSEPR theory=
a model used to predict the geometry of molecules
75
76

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