Chapter 2 A&P Lecture Flashcards
Basic and Inorganic Chemistry
1
Q
Anything that has mass and occupies space?
A
Matter
2
Q
Pull of gravity on mass?
A
Weight
3
Q
What are the 3 states of matter?
A
Solid, Liquid, Gas
4
Q
Which state of matter has a definite shape and volume?
A
Solid
5
Q
Which state of matter has a changeable shape; definite volume?
A
Liquid
6
Q
Which state of matter has a changeable shape and volume?
A
Gas
7
Q
Capacity to do work or put matter into motion?
A
Energy
8
Q
What are the types of energy and their definitions?
A
Kinetic- energy in action
Potential- stored (inactive) energy
9
Q
Can energy be transferred from potential to kinetic energy?
A
Yes
10
Q
What are the forms of energy?
A
Chemical energy
Electrical energy
Mechanical energy
Radiant or electromagnetic energy
11
Q
What form or energy is stored in bonds of chemical substances?
A
Chemical energy
12
Q
What form or energy results from movement or charged particles?
A
Electrical energy
13
Q
What form or energy is directly involved in moving matter?
A
Mechanical energy
14
Q
What form or energy travels in waves (e.g. visible light, ultraviolet light, and x-rays)?
A
Radiant or electromagnetic energy
15
Q
Can energy be converted from one form to another?
A
Yes
16
Q
Is energy conversion efficient?
A
No, because some energy is “lost” as heat (partly unusable energy)
17
Q
Matter is composed of?
A
Elements
18
Q
True or False: Elements cannot be broken into simpler substances by ordinary chemical methods.
A
True; elements CANNOT be broken into simpler substances by ordinary chemical methods.
19
Q
What are the unique properties of an element?
A
Physical properties and Chemical Properties
20
Q
Define physical properties
A
Physical properties are detectable with our senses or are measurable.
21
Q
Define Chemical properties
A
Chemical properties are how atoms interact (bond) with one another.
22
Q
What are the unique building blocks for each element?
A
Atoms
23
Q
What gives each element its physical and chemical properties?
A
Atoms
24
Q
True or False: Atoms are the smallest particles of an element with properties of that element.
A
True: Atoms are the smallest particles of an element with properties of that element.
25
What is an atomic symbol?
One or Two letter chemical shorthand for each element often the first letter of the element's name.
26
What are the 4 elements that make up 96.1% of body mass?
Carbon -C
Hydrogen -H
Oxygen -O
Nitrogen -N
27
What re the 9 elements that make of 3.9% of body mass?
```
Element: Atomic Symbol:
Calcium Ca
Phosphorus P
Potassium K
Sulfur S
Sodium Na
Chlorine Cl
Magnesium Mg
Iodine I
Iron Fe
```
28
What are the trace elements (found in very minute amounts) found in the body?
```
Chromium Cr
Copper Cu
Fluorine F
Manganese Mn
Silicon Si
Zinc Zn
```
29
What are atoms composed of?
Subatomic particles: Protons, Neutrons, Electrons
30
What subatomic particles are found in the nucleus?
Protons and neutrons
31
Which subatomic particle orbits the nucleus in the electron cloud?
Electrons
32
What makes of almost the entire mass of the atom?
The nucleus
33
Do neutrons or protons carry a charge?
Protons, which have a positive charge. Neutrons carry no charge.
34
What is the mass of a neutron?
Neutron mass = 1 atomic mass unit (amu)
| Proton mass = 1 amu
35
What charge does an electron have when in orbitals within electron cloud?
Electrons carry a negative charge
36
What is the mass of an electron when in orbitals within electron cloud?
1/2000 (0 amu)
37
Are the number of protons usually equal to electrons?
Yes, they are equal in an atom of an element.
38
Which model of an atom is depicted with probable regions of greatest electron density (an electron cloud) and is useful for predicting chemical behavior of atoms?
The Orbital Model - current model used by chemists
39
Which model of an atom incorrectly depicts a simplified and fixed circular electron paths?
Planetary model -used for illustrative purposes in textbooks only and is outdated with the onset of the Orbital model.
40
What determines what an element IS?
The number of protons, the atomic number of an element. 47 protons will Always be Silver.
41
How is a mass number determined?
By adding the total number of Protons + Neutrons in the nucleus. This is the total mass of an atom.
42
How is the mass number depicted?
Written as superscript to left of atomic symbol
| Ex. 7th power Li
43
The number of protons in the nucleus is the ...?
Atomic number
44
How is the atomic number depicted?
Written as subscript to left of atomic symbol
| Ex. tiny 3 below the line Li
45
What is a structural variation of atoms?
Isotopes
46
How do isotopes differ from their original element?
They differ in the number of neutrons they contain, and their atomic numbers remain the same while their mass number is different
47
What are heavy isotopes that decompose to more stable forms and can be detected with scanners?
Radioisotopes
48
What is the term for spontaneous decay?
Radioactivity
49
What is the atomic symbol for Carbon?
C
50
What is the atomic symbol for Hydrogen?
H
51
What is the atomic symbol for Oxygen?
O
52
What is the atomic symbol for Nitrogen?
N
53
What is the atomic symbol for Phosphorous?
P
54
What is the atomic symbol for Sulfur?
S
55
What is the atomic symbol for Calcium?
Ca
56
What is the atomic symbol for Iron?
Fe
57
What is the atomic symbol for Sodium?
Na
58
What is the atomic symbol for Potassium?
K
59
What is the atomic symbol for Chlorine?
Cl
60
What is the atomic symbol for Magnesium?
Mg
61
What is the atomic symbol for Chromium?
Cr
62
What is the atomic symbol for Iodine?
I
63
What is the atomic symbol for Cobalt?
Co
64
What is the atomic symbol for Fluorine?
F
65
What is the atomic symbol for Vanadium?
V
66
What is the atomic symbol for Selenium?
Se
67
What is the atomic symbol for Manganese?
Mn
68
What is the atomic symbol for Copper?
Cu
69
What is the atomic symbol for Zinc?
Zn
70
What is the atomic symbol for Silicon?
Si
71
What is the atomic symbol for TIn?
Sn
72
What is the atomic symbol for Molybdenum?
Mo
73
A stable atom has the same number of...?
Protons and electrons
74
of protons determines an element's...?
Atomic Number
75
An atom that has either gained or lost electrons is called?
An ion
76
An atom that has gained electrons is called?
A negative ion/Anion
77
An atom that has lost electrons is called?
A positive ion/cation
78
2 or more of the same kind of atoms joined by chemical bonds?
Molecules
79
2 or more of different types of atoms proportions designated by a chemical formula is called
A compound
80
An atom that has gained electrons is called?
The electron acceptor which is now a negative ion/Anion
81
An atom that has lost electrons is called?
The electron donor which is now called a positive ion/cation
82
What makes the nucleus positively charged overall?
Because protons are positively charged and neutrons have not charge.
83
The number of protons is always equal to the # of electrons in an atom, so the atomic # indirectly tells us the # of _____ in the atom as well.
Electrons
84
To figure out the number of protons, look at the ?
Bottom subscript, the atomic number. The atomic number is the number of protons.
85
To figure out the number of electrons, look at the
Bottom subscript, the atomic number since in a neutral atom, the number of protons and electrons are the same number.
86
How to figure out the number of neutrons?
Subtract the top number (mass number) from the bottom number (atomic number) to find the number of neutrons.
87
What are elements that have the same number of protons (and electrons), but differ in the # of neutrons they contain?
Isotopes
88
Elements shown on the periodic table usually represent
The most abundant types/forms of an element.
89
What subatomic particle does not change in isotopes?
The number of protons the element has, otherwise, Carbon would not be Carbon, for example.
90
What is another way that isotopes can be written?
Carbon : C-14 to represent the mass number instead of the top subscript.
91
How many neutrons does the carbon isotope C-12, C-13, and C-14 have, respectively when Carbon has 6 protons?
C-12 has 6 neutrons,
C-13 has 7 neutrons,
C-14 has 8 neutrons
Subtract the atomic mass from the atomic number to find the number of neutrons.
92
What is the definition of a "molecule of an element"
A molecule that has more than one of the same element such as 2 Oxygen atoms comboned, shown as O2 or 8 Sulpfur atoms: S8 (the number is a bottom subscript).
93
When two more more DIFFERENT kinds of atoms bind...
...they form a compound such as H2O or CH2
94
Just as an atom is the smallest particle of an element, a molecule is the smallest particle of a
Compound. Compounds are therefore chemically pure.
95
What is the definition of a "molecule of an element"
A molecule that has more than one of the same element such as 2 Oxygen atoms combined, shown as O2 or 8 Sulfur atoms: S8 (the number is a bottom subscript).
96
3 types of mixtures are
Solutions, Colloids, Suspensions
97
When two or more DIFFERENT kinds of atoms bind...
...they form a compound such as H2O or CH2
98
Define hetergenous mixture
A mixture that contains dissimilarities in different areas of the mixture. Randomly selected areas would differ from other areas of the mixture.
99
The substance found in the greatest amount within a mixture is called?
The solvent.
100
The substance in smaller amounts of the mixture/
The solute.
101
In the body, most Solutions are ___?
True solutions containing gases, liquids and solids dissolved in water. Usually transparent that do not scatter light e,g. atmospheric air or saline solution.
102
If glucose is dissolved in blood, the glucose would be the ____ and the blood would be the ____.
Solute
| Solvent
103
Concentration of true solutions can be expressed as:
Percent of solute in total solution (assumed to be water)
Milligrams per deciliter (mg/dl)
Molarity, or moles per liter (M)
104
Percent of solute in total solution (assumed to be water)?
Parts solute per 100 parts solvent
105
Molarity, or moles per liter (M)?
1 mole of an element or compound = Its atomic or molecular wight (sum of atomic weights ) in grams
1 mole of any substance contains 6.02 x 10 to the 23rd power molecules of that substance (Avogadro's number).
106
A mixture that is hetergenous with large solute particles that do NOT settle out
Colloids a,k,a Emulsions.
| Some undergo sol-gel transformations e.g. cytosol during cell divison.
107
A mixture that is heterogenous and has large visible solutes that settle out.
Suspensions such as blood
108
Mixture or Compound? No chemical bonding between components.
Mixture
109
Mixture or Compound? Chemical bonding between components.
Compound
110
Mixture or Compound? Can be separated by physical means such as straining or filtering
Mixture
111
Mixture or Compound? Can be separated only by breaking bonds
Compounds
112
Mixture or Compound? can be either Hetergenous or homogenous.
Mixture
113
Mixture or Compound? All all homogenous
Compound
114
Nuclear attraction is strongest between the positively charged nucleus and the negatively charged electrons.. where/
The closer the electrons are located to the nucleus, the stronger the pull toward it. The further it is away from the nucleus, the more likely it is to chemically interact with other atoms.
115
Define the rule of eights.
The outermost shell, called the valance shell, is not stable until it has 8 electrons.
116
What makes an atom chemically inert?
If the valence shell has 8 electrons. Noble gasses such as helium and neon are inert.
117
Most ionic compounds are ____?
Salts. When dry salts form crystals instead of indie molecules. Example: NaCl (Sodium Chloride).
118
What happens to the two ions after electron transfer?
They become attracted to each other since they are now oppositely charged, and combine to form an ionic bond such as Sodium chloride.
119
What happens to the two ions after electron transfer?
They become attracted to each other since they are now oppositely charged, and attract to form an ionic bond such as Sodium chloride.
120
A bond formed when two or more electrons are shared between atoms to achieve stability.
Covalent bond.
121
The type of covalent bond where electrons are shared equally, and produces electrically balanced, nonpolar molecules such as CO2
Nonpolar covalent bonds. They always appear linear and symmetrical
122
The type of covalent bond that is the unequal sharing of electrons which produces polar (aka dipole) molecules such as H2O
Polar covalent bonds. The molecules always look v-shaped bc it has 2 poles of charge - a slightly more negative oxygen end and a slightly more positive hydrogen end.
123
Small atoms with 6 or 7 valances shell electrons which create a strong electron attracting ability are _______?
Electronegative e.g. oxygen
124
Most atoms with 1 or 2 valance shell electons which create a weaker ability to attract and often cause them to lose electrons are _______
Electropositive e.g. sodium
125
The type of covalent bond where electrons are shared equally, and produces electrically balanced, nonpolar molecules such as CO2, and always appear linear and symmetrical.
Nonpolar covalent bonds.
126
Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule
Hydrogen bond
127
Bond which does not offer a true bond but acts mostly as intramolecular bonds, holding a large molecule in a 3D shape. Commonly between dipoles such as water.
Hydrogen bond
128
A chemical reaction that is constructive is called
Anabolic
129
A chemical reaction that is destructive is called
Catabolic
130
What happens in an exergonic reaction?
Energy is liberated
131
What happens in an endergonic reaction?
Energy is absorbed
132
If reaction conditions remain unchanged, all chemical reactions eventually reach a state of
Chemical equilibrium
133
What are some things that increase reaction rate?
Higher temp
Presence of catalysts
The smaller the reacting particles are
134
What is the single most abundant compound in the body which absorbs and releases heat slowly, acts as a universal solvent, participates in chemical reactions, and cushions body organs?
Water
