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| Definite volume and fixed shape |
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| Definite volume and shape takes shape of container |
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| Neither a fixed volume or shape |
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| Pure substances and the two types of pure substances |
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| Elements or compounds, a type of matter that has a definite, or fixed composition that does not vary from one sample of substance to another sample of the same substance |
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| Element and how it's identified |
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Cannot be decomposed into simpler substances
identified by its symbol |
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| Constant composition that can be broken down into its elements by chemical processes |
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| Mixtures and the two types of mixtures |
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two or more substances that can be separated by purely physical means (no fixed composition)
Homogeneous and heterogeneous |
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| the composition and physical properties vary from one part of the mixture to another |
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| or a solution, a mixture uniform in its properties throughout given samples |
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| Three methods of separation of a mixture |
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| Distillation, filtration, chromatography |
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| Separation of a liquid mixture via different methods of vaporization depending on what the components are |
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| Used when the mixture is solid and liquid |
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| This method takes advantage of differences in solubility and/or extent of absorption on a solid surface |
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| Scientific measurements are expressed in the __________ |
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| Unit of mass, length, time, and temperature |
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| Kilogram, meter, second, Kelvin |
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| the force of gravity on an object |
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| the factor that determines the direction of heat flow |
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| Significant figures and when they apply |
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digits in a measured number that include all certain digits plus a final one having some uncertainty
Apply only to measurements, which are quantities subject to error |
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| When do nonzero integers count as significant figures? |
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| When do leading zeros count as significant figures? |
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| When do captive zeros count as significant figures? |
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| When do trailing zeros count as significant figures? |
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| Only when the number contains a decimal point |
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| When a number an exact number? |
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| When we count items or when they arise from definitions |
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| When multiplying or dividing numbers, how do we use sig figs? |
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| We use the least number of significant figures a measurement has |
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| When adding or subtracting numbers, how do we sue sig figs? |
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| We use the least number of sig figs a measurement has |
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| a characteristic of a material involving its chemical change |
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| Physical property and two types of physical properties |
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| a characteristic that can be observed for a material without changing its chemical identity, extensive and intensive |
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| one whose magnitude depends on the quantity of material (mass and volume) |
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| magnitude is independent of the amount of material (density and boiling point) |
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| the ratio of mass to volume |
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| maximum amount of a pure substance (solute) that will normally dissolve in a given quantity of a dissolving medium (solvent) at a given temperature, yielding a solution |
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| in equilibrium with respect to a given dissolved substance |
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| a solution not in equilibrium with respect to a given dissolved substance and in which more of the substance can dissolve |
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| a solution that contains more dissolved substance than a saturated solution |
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| The Atomic Theory, whose theory it is |
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Definition
Dalton's Theory
1) all matter is composed of small, indivisible particles called atoms (false, subatomic particles)
2) all atoms of a given chemical element are identical in mass and in all other properties (false, different masses, isotopes)
3) different chemical elements have different kinds of atoms, and such atoms have different masses
4) in an ordinary chemical reaction, atoms move from one substance to another, but no atom of element disappears or is changed into an atom of another element
5) the formation of a compound from its elements occurs through the combination of atoms of unlike elements in small whole number ratios |
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| Law of conservation of mass |
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Definition
| total mass remains constant during a chemical reaction |
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| Law of constant composition |
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Definition
| in a compound, the proportions by mass of the elements that compose it are fixed |
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| Law of multiple proportions |
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| two or more compounds of the same two elements, the masses of one element that combine with a fixed mass of the second element are in the ratio of small whole numbers |
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| Atomic number and letter used to represent it |
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| Z, number of protons, all atoms of the same element have the same number of protons in the nucleus |
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| Mass number and letter used to represent it |
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| A, sum of protons and neutrons in the nucleus |
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| Same number of protons but different number of neutrons |
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A V
Z /\ (thats an x lol the element symbol) |
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| Atomic mass and how it's expressed |
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| weighted average of the masses of the naturally occurring isotopes of that element, expressed in amu (atomic mass units) |
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| used to determine the types of isotopes present in an element, the exact atomic masses of these isotopes, and the relative amount of each isotope present |
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| found my multiplying the atomic mass of each isotope by its fractional abundance and adding the values obtained |
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Definition
convenient number to use when working with atoms, molecules, or ions (6.0221415e+23)
Represents the number of atoms of an element in a sample whose mass in grams is numerically equal to the atomic mass of the element |
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| 1, 2, 13, 14, 15, 16, 17, and 18 |
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10 elements in center
Periods 4-6 Groups 3-12 |
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Definition
Lithium (Li), sodium (Na), potassium (K), Rubidium (Rb), Cesium (Cs), and francium (Fr)
active elements that readily form ions with a +1 charge when they react with nonmetals |
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Definition
Beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra)
Form ions with a 2+ charge when they react with nonmetals |
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| Group 17- flourine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At) |
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| Group 18- helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn) |
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B, Si, Ge, As, Sb, Te
Have chemical behaviors in between metals and nonmetals
Semiconductors of electricity |
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Definition
Left side of the table and the metalloids line
Solids (besides mercury) and conduct electricity, are ductile, malleable, and can form alloys |
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Right of the stairway
Wide variety of properties
Besides graphite and a form of carbon, non conduct electricity |
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| Which group in the periodic table has one metalloid and no nonmetals? |
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| Which group in the periodic table has no nonmetals or transition metals? |
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Definition
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| Which group in the periodic table has no metals or metalloids? |
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Definition
| forces that hold atoms together in compounds |
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| Covalent bonds, what they're known as, and what kind of atoms form this bond |
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Definition
Bond formed by sharing electrons
Molecules
Two nonmetal atoms |
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| Ionic bonds, what they're known as, and what kind of atoms form this bond |
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Definition
Bond exists between a positive and negative ion
Ionic compounds
A metal and a nonmetal atom |
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Definition
| An assembly of two or more atoms that bind tightly |
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| Involves the types of atoms present (symbols for the elements) and the relative number of atoms (using subscripts) |
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Individual bonds are shown
Emphasizes the connectivity of atoms and chemically important groups of atoms in the molecule |
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| Condensed structural formula |
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Definition
| Suggests the bonding pattern and highlights the presence of a reactive group of atoms |
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| The charged particles formed when atoms lose or gain electrons in chemical reactions |
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Definition
| Positively charged ions (losing electrons, metals) |
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| Negatively charged ions (gaining electrons, nonmetals) |
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| Monoatomic ions and what groups form what |
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Simple ions, single atoms that lost or gained electrons
Metals in groups 1 and 2 form positive ions with a charge equal to their group number
Metals in group 13 form positive charges with a charge equal to the last digit of their group number |
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Definition
| Two or more atoms bonded together |
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| Strong electrical forces between oppositely charged ions that hold ionic compounds together |
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| Typical ionic compound characteristics |
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Definition
Solids at room temperature and do not conduct electricity (molten ionic compounds do)
high melting points
many ionic solids dissolve in water |
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Definition
Compounds whose aqueous solutions conduct electricity
All ionic compounds that are soluble in water are good electrolytes |
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Definition
| Sugar and other molecular solutes |
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| Determining charges of cations from Group 1 and Group 2 |
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Definition
| Form a positive ion with a charge equal to the group number of the metal |
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| Determining charges of cations that are transition metals |
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Definition
| No easily predictable pattern of behavior occurs |
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Term
| Determining charges of nonmetal ions and why |
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Definition
| Negative charge equal to 18 minus the group number of the element because this represents the number of electrons gained by an atom of the element |
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| Determining charges of noble gases in chemical reactions |
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Definition
Very stable
May lose or gain electrons in few reactions |
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| Naming a positively charged monoatomic ion |
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Definition
| Name of the metal plus "ion" |
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| What type of metals form more than one type of positive ion and how are they identified? |
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Definition
Transition metals that can form more than one cation
Roman numeral in parentheses right after metal's name
the ion with the higher charge has a name ending in -ic
the ion with the lower charge has a name ending in -ous |
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Term
| How to name a monoatomic negative ion |
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Definition
| Add -ide to the stem of the name of the nonmetal element from which the ion is derived from |
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| What do most polyatomic anions contain and how do you name them? |
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Definition
Most contain one or more oxygen atoms called oxoanions
Two members in such a series:
smaller number of O atoms ends in -ite
larger number of O atoms ends in -ate
More than two oxoanions make up a series:
hypo- (less than)
per- (more than) |
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| When naming ionic compounds, what ion name is given first? |
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| Positive ion, then negative ion |
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| Rules for naming binary molecular compounds |
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Definition
First element:
Full element name (mono prefix isn't used)
Second element:
Replace ending with -ide
Prefixes designate number of atoms present |
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| Relative proton mass in amu |
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Definition
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| Relative neutron mass in amu |
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| Relative electron mass in amu |
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