DIAGNOSTIC STUDY SET Flashcards
(218 cards)
1
Q
Energy (e)
A
The ability to do work.
2
Q
Kinetic Energy (KE)
A
The energy of motion.
3
Q
Kinetic Energy math formula
A
mass*velocity squared/ 2
4
Q
Potential Energy (PE)
A
The Energy of Position condition and shape.
5
Q
Potential Energy math formula
A
PE= massgravityheight
6
Q
Mechanical Energy (ME)
A
The total energy of motion and position.
7
Q
Mechanical Energy math formula
A
ME= PE+KE
8
Q
Thermal Energy (TE)
A
The total kinetic energy of all the particles that make up the whole object.
9
Q
Chemical Energy (CE)
A
The energy of a compound changing as the rearranging of its atoms to form new compounds.
10
Q
Electric Energy (EE)
A
The energy of moving electrons.
11
Q
Sound Energy (SE)
A
Caused by the vibration of objects.
12
Q
Light Energy (LE)
A
Produced by the vibrations of electrically charged particles.
13
Q
Nuclear Energy (NE)
A
Energy associated with changes in the nucleus of an atom.
14
Q
Nuclear Fission
A
The process of a neutron splitting the nucleus.
15
Q
Chain Reaction
A
A continuous series of fission reactions.
16
Q
Nuclear fusion
A
The combination of two nuclei.
17
Q
The Law of conservation of energy
A
Energy cannot be created or destroyed under ordinary circumstances.
18
Q
Solid
A
Definite shape, definite volume, particles vibrate in place.
19
Q
liquid
A
Particles slide past each other, definite volume, takes shape of container.
20
Q
Gas
A
Particles break away completely from each other, particles move independently of one another, takes shape of container, compressible.
21
Q
Plasma
A
Does not have a definite shape or volume, conducts electric current, admits light.
22
Q
Physical property
A
Matter can be observed or measured without changing the identity of the matter.
23
Q
Physical property examples
A
Color, state, odor, volume, mass.
24
Q
Physical change
A
Change that affects one or more physical properties. It still maintains its original self.
25
Physical change examples
Breaking chalk, freezing water, cutting your hair.
26
Chemical property
Describe a substance based on its ability to change into a new substance with different properties.
27
Chemical property examples
Flammable, reacts with oxygen.
28
Chemical change
Occurs when one or more substances are changed into entirely new substances with different properties. (Can't put back together with fingers.)
29
Chemical change examples
Baking a cake, soured milk.
30
Clues for chemical change
Color change, fizzing/foaming, heat, production of sound, light, new odor.
31
Element
A pure substance that cannot be separated into simpler substances by physical means.
32
Compound
A pure substance composed of 2 or more substances that are chemically combined.
33
Mixture
A compound of 2 or more substances that are not chemically combined.
34
Similarities between compounds and mixtures.
Both are made up of 2 or more materials, but compounds cannot be separated by physical means and a mixture can.
35
Similarities between elements and compounds.
Both cannot be separated by physical means, but a compound is made of 2 or more materials, and an element is not.
36
Change of state
The conversion of a substance from one physical form to another.
37
Melting point
The temperature at which the substance changes from a solid to a liquid. (32 degrees fahrenheit, 0 degrees celsius.)
38
Freezing point
The temperature at which changes a liquid into a solid.
39
Boiling point
The temperature at which a liquid boils. (212 degrees fahrenheit, 100 degrees celsius.)
40
Condensation point
The state changes at which a gas becomes a liquid.
41
Condensation
Change of state from gas to a liquid.
42
Condensation example
Mirror.
43
Sublimation
Change of state from a solid directly to a gas.
44
Sublimation example
Dry ice.
45
Atom
The smallest particle into which an element can be divided and still be the same substance.
46
Atom Charge
Neutral/no charge
47
Nucleus
The tiny extremely dense, positively charged region in the center of an atom. (Has Protons and Neutrons)
48
Protons
The positively charged particles in the nucleus (CANNOT CHANGE THE AMOUNT OF PROTONS)
49
Neutrons
The particles in the nucleus that have no charge.
50
Electrons
Subatomic particles which orbit the nucleus of an atom and are negatively charged. Electrons are found outside the nucleus.(Virtually no mass)
51
Quarks
The smaller particles that make up protons and neutrons.
52
Quark Charge
Neutral/no charge
53
Isotope
An atom that has a different number of neutrons than usual. (Almost every atom)
54
An-Ion
Negative/gained electrons
55
Cat-Ion
Positive/lost electrons
56
Electron Energy
Any of the several different regions in which electrons travel about the nucleus.
57
Valence Shell
The outermost energy level around the nucleus.
58
Valence Electrons
Electrons which are only found in the valence shell. (Atomic number -2)
59
Atomic Mass Unit
The SI unit used to express the masses of particles in an atom.
60
Atomic Number
The number of protons in the nucleus.
61
Mass Number
The sum of the protons and neutrons in an atom.
62
Atomic Mass
The weighted average of the masses of all the naturally occurring isotopes of an element.
63
Metals
Found to the left of the zigzag line. (Solid at room temp, shiny and malleable, good conductor.)
64
Non-Metals
Found to the right of the zigzag line. (Most gasses at room temp, not malleable or shiny, poor conductors.)
65
Metalloids
Also called semiconductors, found at the border of the zigzag line. have properties of both metals and non metals.
66
Groups
Vertical columns of the elements on the periodic table. (Top to bottom.)
67
Periods
Horizontal rows of elements on the periodic table. (Side to Side)
68
Malleable
The ability of a metal to be hammered or rolled into a flat sheet.
69
Ductile
The ability of a metal to be pulled out, or drawn into a long wire.
70
Mendeleev
Periodic table by atomic masses.
71
Moseley
periodic table by atomic number.
72
periodic law
The chemical and physical properties of the elements and periodic functions of the atomic number.
73
Reactivity
The destruction of metal through rusting.
74
Corrosion
The ease and speed with which an element combines or reacts with other elements and compounds.
75
First 13 elements
Hydrogen, Helium,Lithium, Beryllium,Boron,Carbon,
Nitrogen,Oxygen,Fluorine,Neon,Sodium, Magnesium,Aluminum.
76
What are the families (from left the right.)
Alkali metals, Alkaline earth metals, Transitional metals, Lanthanides, Actinides, Metals, Metalloids, Non-Metals, Halogen, Noble gasses.
77
How do atoms bond?
by gaining losing or sharing electrons to have a filled outermost energy level. (Valence shell)
78
Ionic bond
Force of attraction between opposing charged Ions. (Transfered or taken) Ionic bonds = metal+ nonmetal. Ionic bonds are also called metallic bonds.
79
Ions
An atom that has a different number of electrons than usual. Charged particles that form during chemical changes when one or more valence electrons transfer from one atom to another.
80
Covalent bonds
A force of attraction between the nuclei of atoms and electrons shared by the atoms. covalent bonds are also called molecular bonds. (Shared) Non-metal+Non-metal Metalloid+Non-metal.
81
Molecule
A neutral group of atoms held together by covalent bonds.
82
Binary compounds
A compound which is composed of 2 elements.
83
Law of conservation of mass/matter
In a chemical reaction no mass is lost or gained
84
Synthesis reaction
A reaction in which two or more substances combine to form a single compound.
85
Synthesis reactions examples
Sodium reacting with chlorine to form sodium chlorine.
86
Decomposition reaction
A reaction in which a single compound breaks down to form two or more simpler substances.
87
Decomposition reaction examples
The break down of water into hydrogen and oxygen by process called electrolysis.
88
Single replacement reaction
a reaction in which an element takes the place of another element that is part of a compound
89
Single replacement reaction example
Zinc reacting with hydrochloric acid to form zinc chlorine and hydrogen gas.
90
Double replacement reaction
A reaction in which ions in two compounds switch places.
91
Double replacement reaction example
Sodium chloride reacting with silver fluoride to form sodium fluoride and precipitate silver chloride.
92
Exothermic reaction
A chemical reaction in which energy is released or removed.
93
Exothermic reaction examples
Energy released when the chemical of a light stick combine when the stick is cracked
94
Endothermic reaction
A chemical reaction in which energy is absorbed.
95
Endothermic reaction example
Energy being absorbed by the chemicals in an instant ice pack when chemicals are combined.
96
Do metals lose or gain electrons?
Lose
97
Do metals lose or gain electrons?
Gain
98
Four clues of a chemical reaction
1. The formation of gas bubbles. 2. The formation of a solid in a solution. 3. Color change of substance. 4. release or absorb energy of any kind.
99
Precipitate
The formation of a solid in a solution.
100
Acid
Any compound that increases the # of hydrogen ions (H^+) when dissolved in water.
101
Base
Any compound that increases the # of hydroxide ion (OH^-) when dissolved in water.
102
Neutralization
A chemical reaction between an acid and a base solution to become neutral.
103
Indicator
An organic compound that changes color in an acid or a base
104
pH scale
A scale that ranges from 0-14 to determine pH.
105
pH
Potential hydrogen
106
Acid pH
0-6.9
107
Base pH
7.1-14
108
Is an acid corrosive?
Yes
109
Is a base corrosive?
Yes
110
Which has a sour taste?
Acid
111
Which has a bitter taste?
Base
112
Which has a slippery or soapy feel?
Base
113
Which turns blue litmus paper red?
Acid
114
Which turns red litmus paper blue?
Base
115
What happens when they react?
They form salt and/or water
116
What is temperature?
The measure of the average KE of the particles of an object.
117
What is temperatures variables?
Does not vary with mass.
118
What is thermal expansion?
The increase of the volume of a substance due to an increase in the temperature. (Heat makes lower temperature objects expand.)
119
What is the SI unit of temp?
Kelvin=K
120
Freezing temps of water?
32°F, 0°C, 273 K
121
Boiling temps of water?
212°F, 100°C, 373 K
122
What is absolute zero?
The lowest temp on the kelvin scale= 0 kelvin= no particle motion (Called 0K).
123
What is heat?
The process of transferring energy between objects which are at two different temps. The thermal energy ALWAYS goes from the higher temp object to the lower temp object until both objects are at the same temp which is called thermal equilibrium.
124
Heat variables?
Varies with mass and temp and specific heat capacity
125
What is thermal energy?
The total KE of all the particles which make up the whole substance.
126
Thermal energy variables?
Varies with mass and temp.
127
What is the SI unit of thermal energy?
Joules= J
128
What is thermal equilibrium?
When energy is transferred from a higher temp object to the lower temp object until both are at the same temp.
129
What is conduction?
The transfer of energy from one substance to another through direct contact.
130
What is a (Heat) conductor?
Substances that conduct thermal energy very well.
131
Conductor example?
Iron skillet
132
What is an (Heat) insulator?
Substances that do not conduct thermal energy very well.
133
What is convection?
The transfer of energy by the movement (Circulation) of a liquid or a gas.
134
What is radiation?
The transfer of thermal energy through matter or space as waves. (The Sun!)
135
What is thermal conductivity?
The rate at which a substance conducts thermal energy.
136
What is a heat engine?
A machine that uses heat to do work. (2 types)
137
What is an external combustion engine?
To burn fuel outside the engine.
138
External combustion engine example?
Steam engine.
139
What is an internal combustion engine?
To burn fuel inside the engine.
140
Internal combustion engine example?
Car engine.
141
What is a heat pump?
Moves energy to increase or decrease the temperature.
142
What is a heat pump used for cooling?
Energy is taken from the air inside the house and the energy is pumped outside (A.C.) (Inside to outside)
143
What is a heat pump used for heating?
Energy is taken from the air outside the house and the energy is pumped inside. (A Heater) (outside to inside)
144
Law of Electric Charges
States that like charges repel and opposite charges attract.
145
Electric Force
The force between charged objects.
146
Two factors determining the strength of electrical force are?
1: size of the charges
2: distance between charges
147
Conductor (Electrical)
materials in which charges can move easily
148
Insulator (Electrical)
materials in which charges cannot move easily
149
Static electricity
The build up of electric charges on an object. ( An object charges by friction because of the rubbing of two objects together can cause electrons to be whipped from one object and transferred to another)
150
Electric discharge
The loss of static electricity as charges move off an object
151
Electric discharge example
Walking on carpet with your fuzzy socks on, negatively charge builds up on your body. touching a metal door knob.
152
Cell
A device that produces an electrical current by converting chemical energy into electric energy.
153
Battery
A device made up of several cells.
154
Current
The rate at which charge passes through a given point.
155
Current SI unit?
Amps
156
Resistance
The opposition to the flow of electric charge.
157
Electrical power
the rate at which electrical energy is used to do work.
158
Circut
a complete closed path through which electric charges flow.
159
Voltage
the amount of energy released as a charge moves between 2 points in the path of a current
160
What is the SI unit of power?
Watts
161
Magnet
any material that attracts iron or materials containing iron
162
magnetic poles
part of a magnet where the magnetic effects are the strongest
163
magnetic field
exist in the region around a magnet in which magnetic forces can act
164
Electromagnetism
interaction between electricity and magnetism
165
Electromagnet
a magnet that consists of a coil of wire wrapped around an iron core
166
Electric motor
a device that changes electrical energy into KE
167
Ohms law
V=IR
168
Resistance formula
R=V/I
169
Current Formula
I=V/R
170
Motion
an objects change in position over time when compared with a reference point
171
Speed
the rate at which an object moves
172
Velocity
the speed of an object in a particular direction.
173
Velocity formula
d/t plus direction
174
speed formula
d/t
175
speed si unit
m/s
176
velocity si unit
m/s^2
177
acceleration
the rate at which velocity changes
178
calculate acceleration
A= (Vf-Vi)/t
179
Force
a push or a pull
180
force si unit
Newtons
181
Inertia
objects resist any change in motion, Newtons first law
182
what is centrifugal
spin away from center
183
what is centripetal
Spin to center
184
friction
a force that opposes motion
185
Gravity
a force of attraction between objects which is due to their masses
186
weight
a measure of the gravitational force exerted on an object
187
weight si unit
Newtons
188
Mass
the amount of matter in an object
189
mass si unit
Grams
190
Newtons 1st
an object at rest will stay at rest and an object in motion will stay in motion at a constant speed in a straight line unless the object is acted upon by an unbalanced force
191
Newtons 2nd
the acceleration of an object depends on the mass of the object and the amount of force applied
192
2nd law formula
F=ma
193
Newtons 3rd
whenever one object exerts a force on a second object the second object exerts an equal and opposite force on the first
194
Momentum
a property of a moving object that depends on the mass and velocity
195
momentum formula
P=mv
196
Law of conservation of momentum
anytime two or more objects interact, they may exchange momentum, but the total amount of momentum stays the same
197
Machine
a device which helps make work easier by changing the size, direction, or both size and direction.
198
Simple machine
a device that completes a task and makes work easier.
199
work input
the work done ON a machine
200
work output
work done BY a machine
201
mechanical advantage
a number/factor which tells how many times a machine multiplies force.
202
formula for calculating mechanical advantage
MA=output force/input force
203
Efficiency
the measure of how close the machines output is to its input
204
formula for efficiency
Efficiency=(output force/input force)X100=?%
205
lever
machine consisting of a bar that pivots at a fixed point
206
what is the fixed of a lever called
fulcrum
207
inclined plane
a machine which is a straight, slanted surface, ramp.
208
wedge
a machine which consists of a double inclined plane that moves. (Axe)
209
Screw
a machine which is a inclined plane wrapped around a central cylinder
210
wheel and axle
a machine consisting of 2 circular objects of different sizes.
211
pulley
a machine consisting of a grooved wheel which holds a rope or cable
212
Compound machine
a machine that consists of two or more simple machines.
213
work
he action that results when a force causes an object to move in the direction that the force was applied
214
work formula
W=Fd
215
si unit for work
Joules
216
Power
the rate at which work is done
217
Power formula
P=w/t
218
Si unit for power
Watts
