Chemistry Flashcards
1
Q
What does the nucleus of an atom contain?
A
protons and neutrons
2
Q
Nucleus is ____ charged.
A
positively
3
Q
Electrons are ____ charged.
A
negatively
4
Q
An atom becomes an ion when…
A
the number of protons and electrons in an atom is unequal.
5
Q
Protons have a __ charge
A
positive
6
Q
Neutrons have a ___ charge
A
neutral
7
Q
Electrons are ____ times smaller than the proton
A
2000
8
Q
Isotopes are the same element with a different number of ____
A
neutrons
9
Q
Can the proton number change?
A
no
10
Q
atomic mass = ??
A
protons + neutrons
11
Q
the atomic number is the number of ___
A
protons
12
Q
if there are more electrons than protons what will the charge be on the atom?
A
negative
13
Q
if there are more protons than electrons what will the charge be on the atom?
A
positive
14
Q
if the number of protons and electrons are equal then what will the charge be on the atom?
A
neutral
15
Q
cations are atoms that have ___ an electron
A
lost
15
Q
What is an ion?
A
an atom that has gained or lost an electron
15
Q
cations have a ___ charge
A
positive
16
Q
anions are atoms that have ___ an electron
A
gained
17
Q
anions have a ___ charge
A
negative
18
Q
what is an orbital?
A
areas where electrons are likely to be found
19
Q
what is the s orbital
A
spherical area surrounding nucleus
20
Q
how many electrons possible in s orbital
A
2 MAX
21
Q
what is the p orbital
A
dumbbell shape surrounding nucleus
22
Q
how many electrons possible in p orbital
A
6 max
23
what is the d orbital
flower like or hourglass shape surrounding nucleus
24
how many electrons can the d orbital have
10 max
25
what is the f orbital
very irregular shaped orbitals
26
how many electrons can f orbital have
14 max
27
ionic bonds are formed when...
atoms trade electrons in order to achieve stability
28
covalent bonds are formed when...
atoms share electrons in order to achieve stability
29
greater electronegativity = greater____
attraction to electrons
30
low electronegativity means...
lower attraction to electrons
31
the phase of a substance is dependent on two conditions:
temperature and perssure
32
what is condensation?
gas changing to a liquid
33
what is sublimation?
solid changing to a gas
34
what is deposition?
gas changing to a solid
35
how the atom will react depends on the number of ____
valence electrons
36
ionic bonds are formed between..
metal and non metal
37
covalent bonds are formed between..
two non metals
38
what must a substance react to in order for it to be a combustion reaction?
O2
39
what is the product of a combustion reaction?
CO2 + H2O
40
what is the chemical formula of sugar?
C6H12O6
41
what does a catalyst do?
speed up reactions
42
what is it called when a reaction absorbs heat?
endothermic reaction
43
what is it called when a reaction exerts heat?
exothermic reaction
44
what is equilibrium?
rate of forward reaction is equal to rate of backward action
45
what is dynamic equilibrium?
forward and reverse reaction happening at same time
46
what is static equilibrium?
when concentration of reactants and products are not changing
47
if you add a reactant, the position of the equilibrium will shift to the ____.
right
48
if you remove a reactant the position of the equilibrium will shift to the ____ .
left
49
catalysist ___ the activation energy.
lower
50
hydrogen bonding can be achieved through ____ or ____.
adheasion or cohesion
51
what is cohesion?
similar molecule binds to another molecule (water likes water)
52
what is adhesion?
dissimilar molecule binds to another water (water sticks to other things)
53
T or F: hydrogen bonds are strong.
F - H bonds are weak
54
solvent
substance that stuff is being dissolved IN (ex. water)
55
solute
stuff being dissolved
56
what is a neutralization reaction?
reaction between an acid and a base
57
electrons are part of the ___ family.
lepton
58
a polar bond is a ___ type of bond
covalent
59
polar bonds contain...
a positive and negative end
60
when molecules of the same element bind together, they can form ____ or _______ _____.
molecules or crystalline solids
61
covalent bonding occurs with atoms with ____ electronegativities.
similar
62
polar covalent bonds form between...
a highly electronegative atom and a low electronegative atom
63
if two atoms have a difference in electronegativity that is (less than or more than) 0.5, they will form a covalent bond.
less than 0.5
64
if the difference of electronegativity is between 0.5-1.6 then they form a _____.
polar covalent bond
65
if the difference is greater than 2.0 the bond will be ___
ionic.
66
what should you do if the electronegativity is between 1.6-2.0?
check to see if one of the elements is a metal.
67
if the electronegativity is between 1.6-2.0 and one of the elements is metal, what kind of bond is it?
ionic
68
if the electronegativity is 1.6-2.0 and both of the elements are non metals, what kind of bond is it?
polar covalent
69
K-shell
2 electrons
70
L-shell
8 electrons
71
M-shell
18 electrons
72
N-shell
32 electrons
73
How to remember the diatomic elements
Have - Hydrogen
No - Nitrogen
Fear - Fluorine
Of - Oxygen
Ice - Iodine
Cold - Chlorine
Beer - Bromine
74
what are the three types of hydrocarbons?
alkanes, alkenes, alkynes
75
what is a saturated hydrocarbon?
only single bonds
76
what is an unsaturated hydrocarbon?
at least one double or triple bonds
77
alkanes and alkenes are ___ and _____ in water
non polar/ insoluble
78
Which is more reactive: alkanes or alkenes.
alkenes
79
alkynes are the ___ reactive.
most
80
rank alkanes alkenes and alkynes from most to least reactive
alkynes
alkenes
alkanes
81
what is the strongest type of covalent bond?
sigma bond
82
name a covalent bond that is weaker than the sigma bond.
pi bond
83
how are pi bonds formed?
overlap of p orbitals; perpendicular to any sigma bonds
84
what is an ether?
oxygen linking two hydrocarbon groups
85
what is an aldehyde?
oxygen double bound to end of hydrocarbon chain
86
what is a ketone?
oxygen double bound somewhere on the middle f the chain, not the ends
87
Elements on the right side of the table are ___ reactive.
less
88
Elements on the left side of the table are ___ reactive.
more
89
As electrons are added, their attraction to the nucleus ___.
increases
90
What is the most important feature of the periodic table?
periodicity
91
one negatively charged atom and one positvely charged atom form which type of bond?
ionic.
92
speed of evaporation is decreased by
increased atmospheric pressure
93
what are the two types of physical properties
intensive and extensive
94
intensive properties do ___ depend on amount of matter
not
95
extensive properties ___ depend on amount of matter
do
96
what are the intensive properties
color
hardness
melting point
boiling point
density
ductility
malleability
specific heat
temperature
concentration
magnetization
97
what are the extensive properties
volume
mass
weight
energy
entropy
number of moles
electrical charge
98
what is a conductor?
a material that contains moveable electric charges
99
what is the law of conservation of mass?
matter cannot be created nor destroyed
100
how many grams in a kg?
1000
101
how many grams in a liter?
1000
