Earth & Physical Science Flashcards
1
Q
Law of Conservation of Energy
A
energy is not lost but transferred back and forth between kinetic energy and potential energy
e.g. increase in KE will decrease PE
2
Q
a molecule that possesses both positive and negative atomic structure
A
polar molecule
3
Q
a molecule that possesses both positive and negative atomic structure
A
polar molecule
4
Q
involves electron donation to produce a produce a more positive ion
A
oxidation
5
Q
elements
A
susbstances that cannot be broken into simpler types of matter
6
Q
alkene
A
an acyclic unsaturated hydrocarbon that contains one or more C-C double bonds. always end in -ene. (general molecular formula of CnH2n with only one double bond)
7
Q
chemical reactions in living organisms
A
metabolism
8
Q
electron acceptance to produce a more negative ion
A
reduction
9
Q
density
A
ratio of mass per volume of a substance
10
Q
electrons
A
negatively charged subatomic particles found in various energy levels (orbital shells) around the nucles
11
Q
a compound that contains only carbon and hydrogen atoms
these are abundant within living things, foods, fuels and plastics
A
hydrocarbons
12
Q
metals
A
elements that donate highly conductive eletrons to the environment
13
Q
a molecular surface acted upon by an enzyme
A
substrate
14
Q
negatively charged subatomic particles found in various energy levels (orbital shells) around the nucles
A
electrons
15
Q
where atoms are arranged in a highly ordered state
A
crystalline order
16
Q
metabolism
A
chemical reactions in living organisms
17
Q
electrons in the outter most shell
A
valence electrons
18
Q
increase reaction rates by lowering activation energy
these are not consumed in a reaction
A
catalyst
19
Q
substances that are consumed or altered in a chemical reaction
A
reactants
20
Q
electronegativity
A
when 2 atoms form covalent bonds and the covalent bond sharing isnt equal. some atoms “hog” electrons more
attractions for electrons
21
Q
7 visible forms of electromagnetic radiation from long to short wavelengths
A
red, orange, yellow, green, blue, indigo, violet
22
Q
ratio of mass per volume of a substance
A
density
23
Q
metalloids
A
elements that may accept or donate electrons. possess a mixture of metallic and non metallix properties
24
Q
positively charged subatomic particles in the nucleus of an atom
of these distinguishes one atom from another
of these = atomic number
A
protons
25
when 2 atoms form covalent bonds and the covalent bond sharing isnt equal. some atoms "hog" electrons more
attractions for electrons
electronegativity
26
potential energy
the amount of stored energy
energy can be stored in a battery cell or gasoline or gravity can store energy when an object is at a certain height
doubling the height will double this
=mgh
m=mass, g=gravitational constant, h=height
27
atomic mass
the average mass of all known isotopes of an element
it usually represents the most common isotope
28
chemical reactions with a cell
metabolic pathways
29
pH
a measure of hydrogen ion concentation within a solution
30
saturated hydrocarbon with an acyclic carbon atom arrangement. the number of H present are always twice the number of C atoms plus 2 more. e.g. methane (CH4), ethane (C2H6) and propane (C3H8). always end in -ane
they are saturated with H's and have only single bonds
alkane
31
the results of any change in energy
quantified in units Joules and calories
work
32
the amount of heat necessary to cause a phase transition between a liquid and a gas
heat of vaporization
33
study of hydrocarbons and their derivatives. compounds from living organisms
organic chemistry
34
organic chemistry
study of hydrocarbons and their derivatives. compounds from living organisms
35
polar molecule
a molecule that possesses both positive and negative atomic structure
36
an alteration of the physical state between a solid, liquid and gas
phase transition
37
the energy required to raise one unit of mass of a substance by 1 degree C
specific heat
38
radio, microwave, infrared, ultraviolet, x-ray, gamma ray
electromagnetic spectrum divided into bands of wavelengths from long to short
39
atoms with the same number of protons but different numbers of neutrons
isotopes
40
energy is not lost but transferred back and forth between kinetic energy and potential energy
e.g. increase in KE will decrease PE
Law of Conservation of Energy
41
neutrons
neutral subatomic particles in the nucleus of an atom
42
valence electrons
electrons in the outter most shell
43
the energy required to raise one unit of mass of a substance by 1 degree C
specific heat
44
orbital shells
the arrangement of electrons within orbits around the nucleus
45
the flow of energy due to a difference in temperature
heat
46
neutral subatomic particles in the nucleus of an atom
neutrons
47
electron acceptance to produce a more negative ion
reduction
48
energy required to remove an electron from an atom in a neutral state
ionization energy
49
ion
a positively or negatively charged atom
50
used to qualitatively determine pH
do not give precise measurements, just approximations
ex. litmus paper (turns red for acidic solutions and blue for basic solutions)
pH indicator
51
an alteration of the physical state between a solid, liquid and gas
phase transition
52
sharing electrons
covalent bond
53
heat
the flow of energy due to a difference in temperature
54
saturated hydrocarbon with an acyclic carbon atom arrangement. the number of H present are always twice the number of C atoms plus 2 more. e.g. methane (CH4), ethane (C2H6) and propane (C3H8). always end in -ane
they are saturated with H's and have only single bonds
alkane
55
catalyst
increase reaction rates by lowering activation energy
these are not consumed in a reaction
56
crystalline order
where atoms are arranged in a highly ordered state
57
covalent bond
sharing electrons
58
study of hydrocarbons and their derivatives. compounds from living organisms
organic chemistry
59
the amount of stored energy
energy can be stored in a battery cell or gasoline or gravity can store energy when an object is at a certain height
doubling the height will double this
=mgh
m=mass, g=gravitational constant, h=height
potential energy
60
a measure of hydrogen ion concentation within a solution
pH
61
a positively or negatively charged atom
ion
62
alkane
saturated hydrocarbon with an acyclic carbon atom arrangement. the number of H present are always twice the number of C atoms plus 2 more. e.g. methane (CH4), ethane (C2H6) and propane (C3H8). always end in -ane
they are saturated with H's and have only single bonds
63
elements that donate highly conductive eletrons to the environment
metals
64
total number of protons and neutrons found within the nucles of the atom
electrons are not included because they contribute very little mass
mass number
65
ratio of mass per volume of a substance
density
66
energy from Sun reaches Earth in this form
waves of radiation that are characterized by electric and magnetic fields
e.g. gamma, x-ray, ultraviolet, etc
electromagnetic waves
67
ionization energy
energy required to remove an electron from an atom in a neutral state
68
phase transition
an alteration of the physical state between a solid, liquid and gas
69
electromagnetic waves
energy from Sun reaches Earth in this form
waves of radiation that are characterized by electric and magnetic fields
e.g. gamma, x-ray, ultraviolet, etc
70
red, orange, yellow, green, blue, indigo, violet
7 visible forms of electromagnetic radiation from long to short wavelengths
71
latent heat
the amount of energy needed for a phase transition (between solid, liquid and gas)
72
reduction
electron acceptance to produce a more negative ion
73
kinetic energy
amount of energy associated with an object's motion
energy of motion
=(1/2)mv2
v=velocity
74
electromagnetic spectrum divided into bands of wavelengths from long to short
radio, microwave, infrared, ultraviolet, x-ray, gamma ray
75
substrate
a molecular surface acted upon by an enzyme
76
substances that are consumed or altered in a chemical reaction
reactants
77
globular proteins
proteins that are water soluble
78
light-years
the distance that light will travel within 1 year of time
79
metabolic pathways
chemical reactions with a cell
80
reactants
substances that are consumed or altered in a chemical reaction
81
the average mass of all known isotopes of an element
it usually represents the most common isotope
atomic mass
82
the arrangement of electrons within orbits around the nucleus
orbital shells
83
isotopes
atoms with the same number of protons but different numbers of neutrons
84
oxidation
involves electron donation to produce a produce a more positive ion
85
ionic bond
an atom gives an electron to another atom so they both become ions. they bond be cause the ions are attracted to each other
86
the distance that light will travel within 1 year of time
light-years
87
protons
positively charged subatomic particles in the nucleus of an atom
of these distinguishes one atom from another
of these = atomic number
88
pH indicator
used to qualitatively determine pH
do not give precise measurements, just approximations
ex. litmus paper (turns red for acidic solutions and blue for basic solutions)
89
increase reaction rates by lowering activation energy
these are not consumed in a reaction
catalyst
90
the amount of energy needed for a phase transition (between solid, liquid and gas)
latent heat
91
specific heat
the energy required to raise one unit of mass of a substance by 1 degree C
92
acyclic hydrocarbon containing one or more C-C triple bonds
it has a linear (180 degrees) geometry, sp hybridized
nomenclature is same as alkene but with -yne ending
cis/trans are not possible. only constitutional isomers possible
alkynes
93
chemical reactions in living organisms
metabolism
94
proteins that are water soluble
globular proteins
95
mass number
total number of protons and neutrons found within the nucles of the atom
electrons are not included because they contribute very little mass
96
amount of energy associated with an object's motion
energy of motion
=(1/2)mv2
v=velocity
kinetic energy
97
involves electron donation to produce a produce a more positive ion
oxidation
98
a molecular surface acted upon by an enzyme
substrate
99
elements that may accept or donate electrons. possess a mixture of metallic and non metallix properties
metalloids
100
an acyclic unsaturated hydrocarbon that contains one or more C-C double bonds. always end in -ene. (general molecular formula of CnH2n with only one double bond)
alkene
101
an atom gives an electron to another atom so they both become ions. they bond be cause the ions are attracted to each other
ionic bond
102
used to qualitatively determine pH
do not give precise measurements, just approximations
ex. litmus paper (turns red for acidic solutions and blue for basic solutions)
pH indicator
103
susbstances that cannot be broken into simpler types of matter
elements
104
hydrocarbons
a compound that contains only carbon and hydrogen atoms
these are abundant within living things, foods, fuels and plastics
105
a compound that contains only carbon and hydrogen atoms
these are abundant within living things, foods, fuels and plastics
hydrocarbons
106
proteins that are water soluble
globular proteins
107
electrons in the outter most shell
valence electrons
108
the amount of energy needed for a phase transition (between solid, liquid and gas)
latent heat
109
elements that may accept or donate electrons. possess a mixture of metallic and non metallix properties
metalloids
110
heat of vaporization
the amount of heat necessary to cause a phase transition between a liquid and a gas
111
energy required to remove an electron from an atom in a neutral state
ionization energy
112
work
the results of any change in energy
quantified in units Joules and calories
113
alkynes
acyclic hydrocarbon containing one or more C-C triple bonds
it has a linear (180 degrees) geometry, sp hybridized
nomenclature is same as alkene but with -yne ending
cis/trans are not possible. only constitutional isomers possible
114
the amount of heat necessary to cause a phase transition between a liquid and a gas
heat of vaporization
