Chapter 2 Part 1 Lecture Flashcards
1
Q
Purpose of Ch. 2: (4)
A
- Introduce the language and fundamental concepts of chemistry
- Discuss how matter is organized
- Discuss how chemical bonds form and how chemical reactions occur
- Compare and contrast organic and inorganic compounds
2
Q
3 basic Principles of Chemistry:
A
- Chemistry is the science of structure and interactions of matter
- Matter is anything that has mass and takes up space
- Mass is the amount of matter a substance contains, whereas weight is the force of gravity acting on a mass
3
Q
Chemistry is the science of:
A
is the science of structure and interactions of matter
4
Q
Matter is anything that has
A
anything that has mass and takes up space
5
Q
Mass is the amount of
A
the amount of matter a substance contains, whereas weight is the force of gravity acting on a mass
6
Q
Matter exists in 3 forms:
A
- Solid
- Liquid
- Gas
7
Q
4 elements that make up majority of our bodies:
A
- nitrogen
- oxygen
- carbon
- hydrogen
8
Q
Oxygen symbol
A
O
9
Q
Carbon symbol
A
C
10
Q
Hydrogen symbol
A
H
11
Q
Calcium symbol
A
Ca
12
Q
Nitrogen symbol
A
N
13
Q
Phosphorus
A
P
14
Q
Potassium
A
K
15
Q
Sodium
A
Na
16
Q
Chlorine
A
Cl
17
Q
Magnesium
A
Mg
18
Q
Iron
A
Fe
19
Q
Chemical elements are composed of:
A
Chemical elements are composed of units of matter of the same type called atoms
20
Q
Atoms are the ___units of ___ that retain the ____ and ___of an element
A
Atoms are the smallest units of matter that retain the properties and characteristics of an element
21
Q
Atomic number is the number of:
A
protons in nucleus of an atom
22
Q
Mass number is the number of:
A
Mass number is the number of protons and neutrons in an atom
23
Q
Neutron daltons =
A
Neutron = 1.008 daltons
24
Q
Proton daltons=
A
Proton = 1.007 daltons
25
Electron daltons=
Electron = 0.0005 daltons
26
The atomic mass/weight of an element is:
The atomic mass/weight of an element is the average mass of all its naturally occurring isotopes
27
ion:
an atom that has lost or gained an electron
28
Cation aka
positive ion
29
anion aka
negative ion
30
Molecule
2 or more atoms sharing electrons
31
Compound:
Compound – a substance that can be broken down into 2 or more different elements
32
A chemical bond occurs when:
A chemical bond occurs when atoms are held together by forces of attraction
33
The number of electrons in the valence shell determines:
determines the likelihood that an atom will form a chemical bond with another atom
34
Hydrogen ion symbol and charge:
H+
35
Sodium ion symbol and charge:
Na+
36
potassium ion symbol and charge:
K+
37
Ammonium ion symbol and charge:
NH4 +
38
Magnesium ion symbol and charge:
Mg 2+
39
Calcium ion symbol and charge:
Ca2 +
40
Iron (II) ion symbol and charge:
Fe2 +
41
Iron (III) ion symbol and charge:
Fe3 +
42
Fluoride ion symbol and charge:
F-
43
Chloride ion symbol and charge:
Cl-
44
Iodide ion symbol and charge:
I-
45
Hydroxide ion symbol and charge:
OH-
46
Bicarbonate ion symbol and charge:
HCO3 -
47
Oxide ion symbol and charge:
O2-
48
Sulfate ion symbol and charge:
SO42-
49
Phosphate ion symbol and charge:
PO43-
50
Ionic bond example:
NaCl
51
Donated electron charge:
+ (excess of clothes for donation bin)
52
Accepted electron charge:
- (less clothes so accept more)
53
Ionic bonding is through:
Ionic bonding is through the polarity of two atoms
54
3 Type of covalent bonds:
- Single
- Double
- Triple bonds
55
Example of single covalent bond:
H2
56
Example of double covalent bond:
O2
57
Example of triple covalent bond:
N2
58
Covalent bonds aka
Co dependent bond/couple; both offer something and are inseperable
59
Hydrogen bonds result from:
Hydrogen bonds result from attraction of oppositely charged parts of molecules
60
Hydrogen bonds between water molecules give water___:
Hydrogen bonds between water molecules give water cohesion
61
Cohesion is the tendency of
Cohesion is the tendency of like particles to stay together
62
Hydrogen bonds create:
Hydrogen bonds create surface tension
63
Surface tension is a measure of
Surface tension is a measure of the difficulty of stretching or breaking the surface of a liquid
64
Chemical reactions occur when:
Chemical reactions occur when new bonds are formed or old bonds are broken
65
Reactants=
Reactants are starting substances
66
Products=
Products are ending substances
67
Metabolism is the sum of:
Metabolism is the sum of chemical reactions in the body
68
Energy is the capacity to:
Energy is the capacity to do work
69
Law of conservation of energy:
energy can neither be created nor destroyed but it can be converted from one form to another
70
Potential energy aka
stored energy
71
2 examples of potential energy:
- Raising pen in air
| - When rollercoaster rises to top
72
2 examples of kinetic energy:
- When pen is dropped
| - When rollercoaster drops down
73
Chemical energy:
-energy stored in bonds
74
How do our bodies use chemical energy?:
We use it by breaking it apart
75
Exergonic reactions is the releasing of:
Exergonic reactions is the releasing of energy
76
Endergonic reactions bring ____ in:
Endergonic reactions bring energy in
77
Example of exergonic reaction:
-Combustion
78
Example of endergonic reactions:
-Melting ice; heat is brought in and causing melting
79
Catalysts are used to lower:
-Catalysts are used to lower the activation energy in breaking it apart
80
5 types of chemical reactions:
- Synthesis
- Decomposition
- Exchange
- Reversible
- Oxidation-reduction
81
An example of synthesis reaction:
-Synthesizing reactions together; hydrogen + oxygen = H2O
82
An example of decomposition reaction:
Getting water and breaking it down into hydrogen and oxygen
83
Example of exchange reaction:
When reactants change parts like ions, elements, or atoms
84
Example of reversible reaction:
-reactants to products and can be reversed=
| Sodium chloride+calcium carbonate=sodium carbonate+calcium chloride
85
Oxidation reduction reactions:
- reactions transfer electrons between atoms
| - always occur in parallel (where when one substance is oxidized another is reduced)
86
Oxidation=
loss of electrons and energy release
87
Reduction+
gain of electrons and energy gain
88
Inorganic compounds usually: (2)
Inorganic compounds
- usually lack carbon
- are simple molecules
89
Water is the most ___and ____ inorganic compound in all living things
Water is the most important and abundant inorganic compound in all living things
90
composition of Organic compounds: (3)
- Organic compounds always contain H
- always have covalent bonds
- usually contain O
91
Water is an ideal:
water is an ideal medium
92
What type of molecule is water?
Water is a polar molecule
93
Water solvent or solute?
Water is solvent
94
In a hydrolysis reaction, water is:
In a hydrolysis reaction, water is added to break bonds
95
In a dehydration synthesis reaction, water is:
In a dehydration synthesis reaction, water is removed to make bonds
96
2 thermal properties of water:
Water has a:
- High heat capacity
- High heat of vaporization
97
Water is a ___ ____ of our body fluids and helps ___ ____as membranes and organs slide over one another
Water is a major component of our body fluids and helps reduce friction as membranes and organs slide over one another
98
Mixture:
a combination of elements or compounds that are physically blended together but not bonded together
99
3 types of mixtures are:
- solution
- colloid
- suspension
100
Example of a solution:
-Salt water; light can pass through it
101
Example of a colloid:
-homogenous and cloudy: milk
102
Example of a suspension:
-Cloudy but can be separated: blood
103
HCL; components and acid, base or salt?
- H+ & Cl-
| - acid
104
KOH; components and acid, base or salt?
- K+ & OH-
| - base
105
KCL; components and acid, base or salt?
- K+ & Cl-
| - salt
106
(0)-6 PH =
Acidic
107
7 PH =
Neutral
108
8-(14) PH=
Basic
109
Gastric Juice PH=
1.2-3.0
110
Vaginal fluid PH=
3.5-4.5
111
Urine PH=
4.6-8.0
112
Saliva PH=
6.35-6.85
113
Blood PH=
7.35-7.45
114
Semen PH=
7.20-7.60
115
Cerebrospinal fluid PH=
7.4
116
Pancreatic Juice PH=
7.1-8.2
117
Bile PH=
7.6-8.6
118
Maintenance of body fluid homeostasis is...:
Maintenance of body fluid homeostasis is critical
119
Buffer systems help to regulate pH by converting ____ or ___ into ____or _____
Buffer systems help to regulate pH by converting strong acids or bases into weak acids or bases
120
4 facts about Carbons Compounds:
- always contain carbon
- combine in a variety of shapes
- do not dissolve easily in water
- good source of energy
