LT1 Flashcards
(146 cards)
1
Q
temperature scale that uses the absolute zero of temperature 0°K as the lowest temperature
A
Absolute temperature scale Kelvin
2
Q
the lowest temperature possible, 0°K
A
Absolute zero
3
Q
the closeness of a measurement to the true value of the quantity that is measured
A
Accuracy
4
Q
a substance that yields hydrogen ions when dissolved in water
A
Acid
5
Q
minimum amount of energy required to start a chemical reaction
A
Activation energy
6
Q
Group 1A elements which react with water to make bases called metal hydroxides
A
Alkali metals
7
Q
Group 2A elements which reacts with water to make bases called metal hydroxides
A
Alkaline earth metals
8
Q
an ion with a net negative charge
A
Anion
9
Q
the basic unit of an element that can enter into chemical combination
A
Atom
10
Q
the mass of an atom in atomic mass units
A
Atomic mass
11
Q
a mass exactly equal to 1/12th the mass of one carbon-12 atom
A
Atomic mass units
12
Q
number of protons in an atom
A
Atomic number
13
Q
probable position of an electron according to quantum mechanics
A
Atomic orbital
14
Q
one-half the distance between the two-nuclei in two adjacent atoms of the same element in a metal
A
Atomic radius
15
Q
6.022 x 10^23 = # of particles in a mole
A
Avogadro’s number
16
Q
a substance that yields hydroxide ions (OH-) when dissolved in water
A
Base
17
Q
the temperature at which the vapor pressure of a liquid is equal to the external atmospheric pressure
A
Boiling point
18
Q
unit of energy defined as exactly 4.184 joules; originally defined as the heat needed to raise the temperature of 1 gallon of water 1°C
A
Calorie (cal)
19
Q
most abundant of the four major classes of biomolecules
A
Carbohydrates
20
Q
What are some functions of carbohydrates?
A
- storage & transport of energy
- formation/maintenance(?) of structural components
- maintenance(???) of immune system
21
Q
an ion with a net positive charge
A
Cation
22
Q
a change in the relationships of atoms with the making or breaking of bonds resulting in products with different composition and properties from reactants
A
Chemical change
23
Q
True or false: Chemical changes can be separated by physical means.
A
False
24
Q
energy stored in the structure of atoms and bonds of molecules
A
Chemical energy
25
chemical "words" showing the chemical composition of a compound in terms of the numbers and symbols for the atoms of the elements involved
Chemical formula
26
any property of a substance involves converting the substance into some other substance
Chemical property
27
names given to chemical compounds such as water, sugar, etc.
Common names
28
a substance composed of atoms of two or more elements chemically bonded in fixed proportions
Compound
29
amount of solute present in a given quantity of solvent or solution
Concentration
30
when a substance goes from the gaseous state to the liquid state
Condensation
31
a bond in which electrons are shared by two atoms
Covalent bond
32
compounds with only covalent bonds
Covalent compounds
33
mass divided by volume
Density
34
when molecules go directly from vapor to solid, opposite of sublimation
Deposition
35
a molecule that consists of two atoms
Diatomic molecule
36
subatomic particle that has a very low mass and with a negative electric charge
Electron
37
distribution of electrons among the orbitals in an atom or molecule
Electron configuration
38
substance that cannot be separated into simpler substances by chemical means
Element
39
an expression showing the elements present and the ratios of the different kinds of atoms
Empirical formula
40
processes that absorb heat especially chemical reactions
Endothermic processes
41
capacity to do work or to produce change
Energy
42
process where a liquid changes to a gas; also called vaporization by absorbing heat (what the hell does this mean)
Evaporation
43
processes that give off heat especially chemical reactions
Exothermic processes
44
the elements in a vertical column of the periodic table
Family
45
states that, "Energy can be converted from one form to another, but cannot be created or destroyed."
First Law of Thermodynamics
46
product of mass and acceleration
Force
47
temperature at which the liquid becomes a solid as heat is removed
Freezing point
48
freezing point but added heat
Melting point
49
the lowest energy state of a system
Ground state
50
elements in a vertical column of the periodic table
Group
51
Group 7A; elements include F, Cl, Br, I, and At
Halogens
52
transfer of energy between two bodies that are at different temperatures
Heat
53
states that, "It is impossible to know simultaneously both the momentum and the position of a particle with certainty."
Heisenberg Uncertainty Principle
54
parts of a mixture remain physically separated; can be seen as separate components
Heterogeneous mixture
55
the composition of the mixture, after sufficient stirring, is the same throughout the solution
Homogeneous mixture
56
water-liking molecules which easily dissolve in water
Hydrophilic
57
water-fearing molecules which do not easily dissolve in water and which will separate into layers
Hydrophobic
58
a tentative explanation for a set of observations
Hypothesis
59
a system of units based on metric units
International System of Units
60
an atom or group of atoms that has a net positive or negative charge
Ion
61
atoms having the same atomic number but different mass numbers
Isotopes
62
unit of energy given by newtons*meters
Joule
63
the SI base unit of temperature for absolute temperature measurement
Kelvin
64
energy of motion
Kinetic energy
65
states that, "The total quantity of energy in the universe is constant."
Law of Conservation of Energy
66
states that, "Matter can be neither created nor destroyed."
Law of Conservation of Mass
67
states that, "Different samples of the same compound always contain same elements in the same proportions by mass."
Law of Definite Proportions
68
any fat-soluble, naturally-occurring molecule
Lipids/Fats
69
functions of fats/lipids
- energy storage
| - act as structural components of cell membranes
70
volume of 1,000 cubic centimeters
Liter
71
takes the shape of the container with a fixed volume and thus forms a surface
Liquid
72
amount of matter in an object
Mass
73
total number of neutrons and protons present in the nucleus of an atom
Mass number
74
anything that occupies space & has mass
Matter
75
the temperature at which solid phase becomes liquid phase
Melting point
76
an element which gives or takes electrons and properties intermediate between those of metals and nonmetals
Metalloid
77
elements that give electrons, are good conductors of heat and electricity, form positive ions in ionic compounds, especially metal hydroxides with water
Metals
78
an acid-base reaction between an acid and a base producing salt and water
Neutralization reaction
79
two liquids that are completely soluble in each other in all proportions
Miscible
80
a combination of two or more substances in which the substances retain their identity
Mixture
81
the mass (in grams or kilograms) of one mole of atoms, molecules, or other particles
Molar mass
82
the number of moles of solute in one liter of solution
Molarity
83
a chemical abbreviation showing the exact numbers of atoms of each element in a molecule
Molecular formula
84
Avogadro's number of any substance
Mole
85
at least two atoms in a definite arrangement held together by bonds
Molecule
86
an ion that contains only one atom
Monatomic ion
87
a subatomic particle with no electric charge and great mass slightly greater than a proton's
Neutron
88
SI unit for force
Newton
89
nonmetallic elements in Group 8A whose outer valence shell (p shell) is totally filled
Noble gases
90
elements that take electrons and are usually poor conductors of heat and electricity
Nonmetals
91
On what side of the periodic table are the nonmetals found?
Right side
92
a molecule with no overall separation of different charges
Nonpolar molecule
93
central core of an atom
Nucleus
94
An atom (other than hydrogen) tends to form bonds until it is surrounded by 8 valence electrons.
Octet Rule
95
the positive or negative number of charges an atom would have in a molecule if electrons were transferred completely in the direction indicated by the difference in electronegativity
Oxidation number
96
any substance that takes electrons from another substance thereby increasing the oxidation numbers in another substance
Oxidizing agent
97
the expected positions of moving electrons around the nuclei of an atoms and molecules
Orbital
98
branch of chemistry that deals with carbon compounds
Organic chemistry
99
compounds that contain carbon, usually in combination with elements such as hydrogen, oxygen, nitrogen, and sulfur
Organic compounds
100
a horizontal row of the periodic table
Period/Series
101
a tabular arrangement of the elements
Periodic table
102
a measure of the amount of acidity or H+; specifically the negative logarithm of the hydrogen ion concentration
pH
103
change from one phase to another
Phase change
104
a particle of light
Photon
105
a change in which the physical form/state of a substance, but not its composition, is altered
Physical change
106
covalent bond in which the electron pair is unequally shared, so the bond has partial negative and partial positive poles
Polar covalent bond
107
a molecule that possesses a dipole moment
Polar molecule
108
an ion with more than one atom
Polyatomic ion
109
any molecule composed of more than two atoms
Polyatomic molecule
110
energy of position
Potential energy
111
the closeness of agreement of two or more measurements of the same quantity
Precision
112
force applied per unit area
Pressure
113
the substance formed as a result of a chemical reaction
Product
114
a subatomic particle having a single positive electric charge.
Proton
115
True or false: The mass of a proton is almost 20 times bigger than an electron's mass.
False. The mass of a proton is almost 2,000 times bigger than an electron's mass.
116
large organic compounds made of amino acids arranged in a linear chain and joined together by peptide bonds between the carboxyl and amino groups of adjacent amino acid residues.
Protein
117
energy transmitted in the form of waves
Radiant energy
118
the emission and transmission of energy through space in the form of particles and/or waves
Radiation
119
the spontaneous breakdown of an atom by emission of particles and/or radiation
Radioactivity
120
starting substances in chemical reactions
Reactants
121
any substance that donates electrons to another substance thereby decreasing the oxidation numbers of the second substance
Reducing agent
122
a reaction that can occur in both directions
Reversible reaction
123
any ionic compound which is the product of an acid-base neutralization
Salt
124
states that, "Entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process."
Second Law of Thermodynamics
125
the number of meaningful digits in a measured or calculated quantity
Significant figures
126
has a fixed shape that does not conform to the shape of a container
Solid
127
maximum amount of solute that can be dissolved in a given quantity of solvent at a specific temperature
Solubility
128
the substance present in smaller amount in a solution
Solute
129
a homogeneous mixture of two or more substances
Solution
130
the substance present in larger amount in a solution
Solvent
131
a chemical formula showing how atoms are bonded to one another in a molecule
Structural formula
132
the process in which molecules go directly from the solid to vapor phase
Sublimation
133
matter that has a definite or constant composition (the number and type of basic units present) and distinct properties
Substance
134
one- or two-letter representation of an element
Symbol
135
energy associated with the random motion of atoms and molecules or heat
Thermal energy
136
escape of molecules from the surface of a liquid
Vaporization
137
the force that gravity exerts on an object
Weight
138
any change caused by exerting force or energy
Work
139
Write the number 8,776,700,000 in scientific notation.
8.7767 x 10^9
140
How many significant figures does .00808 have?
3 significant figures
141
How many significant figures does 82,500. have?
5 significant figures.
142
How many significant figures does 0.000 have?
0 significant figures
143
How many significant figures does 1.345000
7 significant figures
144
Convert 69°F to °C. Observe significant figures.
20.°C. i think. sana.
145
What is 9x10^9 * 5x10^14 ?
```
= (9 * 5)*10^(9+14)
= (45)*10^13
= 4.5x10^14
(and bc significant figures)
= 5x10^24
```
146
What is the molar mass of CH4? Use atomic weights H = 1.008, C = 12.01.
16.04 g/mol (i think)
