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| Hydrogen Carbonate (Bicarbonate) |
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Anything that has mass and occupies space;
Solid, liquid, gas;
Solid- Fixed shape and volume
Liquid- Has fixed volume but is not rigid in shape-takes shape of container
Gas-Nor a fixed volume nor a rigid shape |
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| Pure Substances (Fixed composition and a unique set of properties) |
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| Mixtures- Composed of two or more substances |
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Heterogeneous (Coarse)
Homogeneous (Solutions) |
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Type of matter that cannot be broken down into two or more pure substances
113 known elements, 91 occur naturally
Identified by its symbol consisting of one or two letters, usually derived from its name, or latin name |
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A pure substance containing more than one element
eg: Water is a compound of hydrogen and oxygen
Have fixed compositions- A given compound always contains the same elements in the same percentages by mass
To resolve compounds into elements, different methods can be used.
Heat, Electrolysis |
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A mixture contains two or more substances combined in such a way that each substance retains its chemical identity.
Homogeneous- Composition is the same throughout. Another name is solution, made up of solvent, and solute.
Heterogeneous- Composition varies throughout i.e. Rocks.
Many different methods can be used to seperate the components of a mixture.
Filtration, Distillation, Chromatography
All gaseous mixtures including air are solutions |
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1 cm = 10^-2m
1 mm = 10^-3m
1 km = 10^3 m
1 nm = 10^-9m |
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Volume - Cubic centimeters
Liters
Millimeters |
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1 cm(3) = (10^-2m)cubed = (10^-6m) cubed
1 L = (10^-3m) cubed = (10^3cm) cubed
I mL= (10^-3L)= (10^-6m)cubed
1 mL = 1 cm cubed |
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Mass - Grams
Kilograms
Milligrams |
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1 g = (10^-3kg)
1 mg= (10^-3g)
1 Mg= (10^6 g) = (10^3)kg |
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| Measure of the amount of matter in an object |
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Measure of gravitational force acting on the object
Determine mass by weighing |
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Celsius (C)
Kelvin (K)
Fahrenheit (F) |
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| Must be independent of amount |
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| Dependent on amount (mass and volume) |
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| These are observed when the substance takes part in a chemical reaction, which converts it into a new substance. |
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Observed without changing the chemical identity of a substance.
(Melting point, boiling point) |
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The process by which a solute dissolves in a solvent. (Physical)
Number of grams of the substance that dissolves in 100 g of solvent at a given temperature. |
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| The point at which a solution of a substance can dissolve no more of that substance. This point, the saturation point, depends on the temperature of the liquid as well as the chemical nature of the substances involved. |
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| Being able to dissolve more solute. |
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| If a change in conditions (e.g. cooling) mean that the concentration is actually higher than the saturation point, the solution has become supersaturated. |
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| If a change in conditions (e.g. cooling) mean that the concentration is actually higher than the saturation point, the solution has become supersaturated. |
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| John Dalton's Atomic Theory |
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An element is composed of tiny particles called atoms.
In an ordinary chemical reaction, atoms move from one substance to another, but no atoms of any element disappears or is changed into an atom of another element.
Compounds are formed when atoms of two or more elements combine. |
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| Law of conservation of mass |
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| There is no detectable change in mass in an ordinary chemical reaction. If atoms are conserved in a reaction, mass will be conserved. |
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| Law of constant composition |
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| This tells us that a compound always contains the same elements in the same proportions by mass. If the atom ratio of the elements in a compound is fixed, their proportions by mass also be fixed. |
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| Law of multiple proportions |
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| When two elements form more than one compound. In these compounds, the masses of one elementthat combine with a fixed mass of the second element are in ratio of small whole numbers. |
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Carry a negative charge
They are equal to protons
Found in an outer region if an atom where they form what amounts to a cloud of negative charge. |
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Positively charged
Cancel out electrons
Found in the nucleus |
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Neutral charge
In the nucleus |
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Number of protons and electrons
In a neutral atom, protons and electrons are the same |
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| Atoms that contain the same number of protons but a different number of neutrons |
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| Mass number (top), Atomic number (bottom) Element symbol |
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| Horizontal rows in the periodic table |
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| Vertical columns in the periodic table |
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| Group 1 at the far left of the table |
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| Two or more atoms that may combine with one another to form an uncharged molecule.Held by strong forces called covalent bonds. Mostly represented by molecular formulas. |
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| When an atom loses or gains electrons |
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| Metal atoms typically tend to lose electrons to form positively charges ions called cations. |
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| Nonmetal atoms form negative ions by gaining electrons. They are called anions. |
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| The electrical forces between oppositely charged charged ions that hold together compounds. |
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Monoatomic cations take the name of the metal from which they are derived.
Roman numerals to distinguish charge.
Named by adding suffix -ide to the stem of the name of the nonmetal from which they are derived. |
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First word names the cation
Second names the anion |
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| Binary molecular compounds |
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Two nonmetals
First word gives the name of the element w/ Greek prefix
Second word consists of appropriate Greek prefix, stem of the name, the suffix ide. |
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