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66 Cards in this Set
- Front
- Back
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Anything that has mass and takes up space (has volume).
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Matter
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Measure of amount of matter (does not change with location)
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Mass
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Measure of pull of gravity on matter (can change with location)
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Weight
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Matter changes its identity (formula). also called chemical reaction
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Chemical Change
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Matter keeps its identity
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Physical Change
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Law is summary of observations
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Scientific method
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used to respresent very big or very small numbers- uses power of 10
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Scientific Notation (exponential)
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1 in ch equals
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2.54 cm
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1 pound equals
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453.6 grams
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1 quart equals
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0.946 Liters
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1 meter equals
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39.37 inches
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1 mile equals
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1.609 km
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1 oz equals
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28.35 grams
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1 kg equals
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2.205 pounds
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1 gal equals
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3.785 Liters
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1 Liter equals
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33.81 fluid oz
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1 Liter equals
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1.057 quarts
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freezing point of water if 32 degrees and boiling point of water is 212 degrees
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Fahrenheit
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freezing point of water is 0 degrees and boiling point of water is 100 degrees
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Celsius
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Kelvin
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zero is lowest possible temperature
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degrees F -> degrees C
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degree F = 9/5 degree C + 32
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degrees C -> degrees F
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degree C = 5/9 (degree F - 32)
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Kelvin
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degree C + 273
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three states of matter
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gas, liquid, solid
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ratio of mass to volume
m/v |
density
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density of a substance compared to water
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specific gravity
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The capacity to do work
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Energy
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Energy of motion
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Kinetic Energy
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Energy an object has because of its position- stored energy (think of a spring)
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Potential Energy
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KE =
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KE = 1/2 mv^2
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Energy cannot be created nor destroyed
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Law of Conservation of Energy
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True or False: Heat is a form of energy
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True
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1 kcal =
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1 kcal = 1000 cal
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1 cal =
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1 cal = 4.184 J
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The amount of heat necessary to raise the temperature of 1 g of a substance by 1 degree C
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Specific Heat
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The amount of heat change when matter is heated or cooled is given by the following equation
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Amount of heat= SH x Mass x change in temp
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Anything that occupies space and has mass
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Matter
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Fixed composition; cannot be further purified
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Pure substance
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a combination of two or more substances
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Mixture
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cannot be subdivided by chemical or physical means
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Elements
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Elements united in fixed ratios
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Compounds
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Matter uniform composition thrughout
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homogeneous
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matter non uniform composition
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heterogeneous
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Dalton's atomic theory
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all matter is composed of very tiny particles called atoms
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sum of the number of protons plus neutrons in the nucleus of an atom
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mass number
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number of protons in the nucleus of an atom
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atomic number
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mass number is on top
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true
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atomic number is on top
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false
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atoms with the same number of protons but a different number of neutrons
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isotopes
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weighted average of masses of isotopes of an element
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atomic weight
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solids, shiny, conduct electricity, ductile, malleable
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metals
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right side of periodic table, brittle, dull, porr conductors of electricity, accept electrons fo form negative ions
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nonmetals
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semi- metals, some properties of metals, and nonmetals
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metalloids
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elements are arranged in order of decreasing atomic number
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false, increasing
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elements with repeating properties are in the same group or family
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true- collumn or verticle row
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elements in same period change properties as you go across the period
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true, horizontal
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melting and boiling points increase as you go down the table
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false, decrease
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noble gases do not react with other elements, or form ions
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true
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the arrangement of electrons outside the nucleus
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electron configuration
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the energy required to remove the most loosely held electron from and atom in the gaseous state
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ionization energy
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ionization energy is a matter property
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false, periodic
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ionization energy increases as you move from left to right and as you move from bottom to top
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true
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the outermost incomplete shell
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valence shell
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an electron in the valence shell
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valence electron
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electron inside the outermost shell
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core electron
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ground state
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electron configuration of the lowest possible energy- higher than that is excited state
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