Chem Exam #1

Front 1

homogeneous

Back 1

all mixed together equally, all in one phase

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Heterogeneous

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orange juice with pulp, liquid + solid

Front 3

mega- (M)

Back 3

1,000,000 million

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kilo- (k)

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1,000 thousand

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deci- (d)

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0.1 tenth

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centi- ( c)

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0.01 hundredth

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milli- (m)

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0.001 thousandth

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micro- (nu)

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0.000001 millionth

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Density=

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mass/volume

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Celsius to Fahrenheit

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F = (9/5)C + 32

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precision

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how close measurements in a series are to eachother

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accuracy

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how close a measurement is to the actual value

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kinetic energy

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energy due to motion

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potential energy

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energy due to position

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K to C

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C = K - 273.15

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Law of Conservation of Mass

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Mass is conserved in chemical reactions

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Law of Constant Composition

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compounds compositions are the same ANYTIME, ANYWHERE

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Law of Multiple Proportions

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Elements combine in specific rations every time

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Isotope

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atoms with same number of protons, but different numbers of NEUTRONS

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Atomic Number (Z)

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Number of PROTONS

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Mass Number (A)

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number of protons + neutrons

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Isotopic Symbol

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AZ X

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Atomic Mass

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mass of a single atom

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Molecular Mass

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mass of a single molecule (sum of atomic masses of each atom in molecule)

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Formula mass

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the sum of the atomic masses of each atom in a formula unit (ionic compounts, not molecules, but crystalline)

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Average Atomic mass

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Atomic mass when all isotopes and their relative percentages are taken into account

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Covalent Compounds

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Compounds resulting from the sharing of electrons by atoms

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ionic compounds

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compounds composed of positive ions (cations) and negative ions (anions)

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Cation

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positive ion

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Anion

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negative ion

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Covalent Bond

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nonmetal + nonmetal

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Covalent Bond

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Metalloid + nonmetal

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Ionic Bond

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Metal + Nonmetal

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SiCl4 (I or C?)

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Covalent

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LiF (I or C?)

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Ionic

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BaCl2 (I or C?)

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Ionic

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B2H6 (I or C?)

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Covalent

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Na2O (I or C?)

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Ionic

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C2H4 (I or C?)

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Covalent

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Empirical Formula

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Shows the simplest integer ratio of atoms of each element in a compound

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Molecular Formula

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Shows the number of Atoms of ach element in a molecule

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Structural Formula

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Shows the connectivity of the atoms in a molecule

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Formulas of hydrogen peroxide

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Empirical Formula: HO Molecular Formula H2O2

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Naming Ionic Compounds: metals w. only one type of ion

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metal name + nonmetal name with ide suffix NaCl - sodium chloride

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Naming Ionic Compounds: Metals with two or more different ions

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metal name (oxidation state as Roman numeral in parenthesis) + nonmetal name with ide suffix PbO2 - Lead (IV) Oxide

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Naming Ionic Compounds: Hydrates

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name as other ionic compounds except add prefix + hydrate as third word Bacl2 . 2H2O - barium Chloride Dihydrate

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Hydrate

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compound whose crystals contain discrete water molecules (water of hydration)

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Naming Covalent Compounds

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element name with prefix (mono, di, tri… etc) N2O4 - dinitrogen tetroxide

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Covalent Compunds, periodic table position

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both elements from right hand side of periodic table

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mono

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1

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di

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2

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tri

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3

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tetra

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4

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penta

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5

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hexa

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6

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hepta

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7

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octa

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8

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nona

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9

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deca

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10

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Naming Polyatomic Ions

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Compounds of Polyatomic ions are named like binary ionic compounds K2CO3 - potassium carbonate

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Acid

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Yield H+ ions in water

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Binary Aqueous Acids

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acid = 2 elements (aq) = in water

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HCl (aq)

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hydrochloric acid

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HI (aq)

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hydroiodic acid

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H2S (aq)

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hydrosulfuric acid

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HCN (aq)

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hydrocyanic acid

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Naming Binary Aqueous Acids

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hydro + (partial) element name with ic suffix + acid

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Oxoacids

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contain hydrogen, oxygen, and a third element

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Naming Oxoacids

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(partial) element name + suffix + acid

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-ic acids

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-ate anions

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-ous acids

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-ite anions

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H2SO4

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sulfuric acid

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HNO3

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nitric acid

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H2CO3

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carbonic acid

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HClO2

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chlorous acid

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Hydrocarbons

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contain only carbon and hydrogen

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Alkanes

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hydrocarbons with only single bonds

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Compound

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matter composed of two or more different elements chemically bonded together

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mixture

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two or more substances that are physically intermingled

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PT: group

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vertical columns

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PT: period

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horizontal rows

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pt: Metals

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first 2 groups, minus H.. Entire middle section, including removed portion, and elements to the right of the stairstep, including Al and Po

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pt: Nonmetals

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Hydrogen, Plus colums 14-18 on right side of stair step line

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pt: Metalloids

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Elements along both sides of stairstep line, minus Al, Po, At

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pt: elements in a group

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have similar chemical properties

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pt: elements in a period

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have different chemical properties

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diatomic molecules

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N2, O2, F2, Cl2, Br2, I2

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tetratomic molectule

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P4

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octatomic molecules

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S8, Se8

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silver ion

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Ag+

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zinc ion

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(Zn)2+

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cadmium ion

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(Cd)2+

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Chromium

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II & III

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Cobalt

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II & III

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Copper

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I & II

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Iron

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II & III

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Lead

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II & IV

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Mercury

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I & II

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Tin

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II & IV

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Manganese

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II & IV

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Nickle

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II & III

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ammonium

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(NH4)+

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hydronium

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H3O+

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acetate

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CH3COO-

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cyanide

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CN-

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hydroxide

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OH-

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hypochlorite

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ClO-

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chlorite

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(ClO2)-

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chlorate

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(ClO3)-

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perchlorate

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(ClO4)-

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nitrite

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(NO2)-

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nitrate

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(NO3)-

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permanganate

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(MnO4)-

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carbonate

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(CO3)2-

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hydrogen carbonate (bicarbonate)

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(HCO3)-

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chromate

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(CrO4)2-

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dichromate

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(Cr2O7)2-

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peroxide

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(O2)2-

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phosphate

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(PO4)3-

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hydrogen phosphate

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(HPO4)2-

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dihydrogen phosphate

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(H2PO4)-

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sulfite

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(SO3)2-

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sulfate

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(SO4)2-

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hydrogen sulfate (bisulfate)

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(HSO4)-

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1 mole (mol)

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6.022 x 1023

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molar mass

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the mass in grams of one mol of substance

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mass % =

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mass of atoms of element/mass of all atoms x 100

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find empiricle formula of compound with C=44.77% H=7.52% and O=47.71%

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C5H10O4

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s

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solid

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l

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liquid

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g

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gas

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aq

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aqueous

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limiting reactant

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reactant that runs out first and determines final amount

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theoretical yield

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max. possible yield of products, predicted by the balanced equation and reactant quantities

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Theoretical yield of ammonia in the reaction of 25.0 g N2 and 6.00 g H2?

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Theoretical Yield = 30.4 g NH3

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Percent yield =

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actual yield/theoretical yield

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41.5 g bromobenzene from 25.2 g benzene and excess bromine, percent yield?

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81.90%

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What mass of iron(III) oxide will be produced if 12.3 g of iron react with an excess of oxygen according to the reaction, 4F(s) + 3O2(g) --> 2Fe2O3(s)

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a) 4.4 g b) 8.8 g c) 16.7g d) 17.6 g e) 35.2 g

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solution

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a homogenous mixture of two or more substances

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solute

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the solution component present in a smaller amount

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solvent

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the solution component present in a larger amount

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aqueous solution

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a solution with water as solvent and gas, liquid, or solid as solute

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concentration

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amount of solute dissolved in given quantity of solution

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molarity (M) =

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moles of solute/liters of solution

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What volume of 0.246 AgNO3 is required to completely precipitate all of the Cl- in 0.250 L of 0.153 M BaCl2?

Back 145

0.311 L

Front 146

isomers

Back 146

compounds with the same molecular formula, but with different properties (shape, etc.)

Front 147

acid compound is 40.0 mass % C, 6.71 mass % H, and 53.3 mass % O. (a) determine empirical formula (b) determine molecular formula

Back 147

(a) CH2O (b) C3H6O3

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water

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high polarity makes it a good solvent

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electrolytes

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substance that conducts current when dissolved in water

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hydration

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when an ionic compound is dissociated by water ions

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nonelectrolytes

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do not dissociate in water and therefore do not conduct electricity

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strong electrolyte

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dissociates nerly 100% into ions in water

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weak electrolyte

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substance that ionizes only slightly in water

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Aqueous Ionic Reactions: Molecular Equation

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Pb(NO3)2 (aq) + 2 NaBr (aq) --> Pb(Br2) (s) + 2 (NaNO3) (aq)

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Aqueous Ionic Reactions: Total Ionic Equation (split into ions and include spectator ions)

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(Pb)2+ (aq) + 2(NO3)- (aq) + 2Na+ (aq) + 2 Br- (aq) --> (PbBr2) (s) + 2Na+ (aq) + 2(NO3)- (aq)

Front 156

Aqueous Ionic Reactions: Net Ionic Equation (omit spectator ions)

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Pb2+ (aq) + 2Br- (aq) --> PbBr2 (s)

Front 157

K3PO4 (aq) + Ca(NO3)2 (aq) --> Ca3(PO4)2 (s) + ?? Write the net ionic equation for this reaction

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3(Ca)2+ (aq) + 2P(O4)3- (aq) --> Ca3(PO4)2 (s)

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precipitate

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an insoluble solid formed by a reaction in solution

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Solubility Rules: things that are soluble

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1. Common compounds of (1) and ammonium ions 2. Common nitrates, acetates, perchlorates 3. Chlorides, Bromides, Iodides, EXCEPT those of Ag+, (Pb)2+, Cu+, and (Hg2)2+ 4. Sulfates, EXCEPT those of (Ca)2+, (Sr)2+, (Ba)2+, Ag+, and (Pb)2+

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Solubility Rules: things that are not soluble

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1. All metal hydroxides, EXCEPT those of (1) and the larger members of (2) beginning with (Ca)2+ 2. Carbonates and Phosphates, EXCEPT those of (1) and (NH4)+ 3. Sulfides EXCEPT those of (1), (2) and (NH4)+

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Double Displacement: metathesis reactions

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AX + BY --> AY + BX

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Soluble? CuCl2

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Soluble

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Soluble? Mn(OH)2

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Insoluble

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Soluble? Na2Cr2O7

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Soluble

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Soluble? NiSO4

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Soluble

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Soluble? Ca3(PO4)2

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Insoluble

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Soluble? K2S

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Soluble

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Will a precip form? BaCl2 (aq) + Na2SO4 (aq) -->

Back 168

yes

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Will a precip form? CaCl2 (aq) + KC2H3O2 (aq)

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no

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base

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yield OH- in water

Front 171

hydrochloric acid (strong acid)

Back 171

HCl

Front 172

nitric acid (strong acid)

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HNO3

Front 173

sulfuric acid (strong acid)

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H2SO4

Front 174

sodium hydroxide (strong base)

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NaOH

Front 175

potassium hydroxide (strong base)

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KOH

Front 176

acid + base -->

Back 176

salt + water

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titrant

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a solution of accurately known concentration

Front 178

analyte

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a solution of unknown concentration

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equivalence point

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exact titrant volume required to completely react with the analyte

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end point

Back 180

the titrat volume slightly in excess of that required to completely react with the analyte

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24.57 mL of 0.1008 M NaOH are required to neutralize 25.00 mL of HCl. What is the HCl molarity?

Back 181

0.09907 M

Front 182

Bronsted-Lowry Acid

Back 182

a proton donor

Front 183

Bronsted-Lowry Base

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a proton acceptor

Front 184

Oxidation-reduction reaction (redox)

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a reaction in which there is a net movement of electrons from one reactant to or towards another

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oxidation number

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the charge an atom has or would have if all unevenly shared electrons were transferred completely

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on: elemental form

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0

Front 187

on: monatomic ion

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on = ionic charge

Front 188

on: sum of on in compound

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equals zero

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on: (1)

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1

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on: (2)

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2

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on: hydrogen

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+1 when in combination with nonmetals

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on: fluorine

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-1 in combination with metals and boron

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on: oxygen

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-1 in peroxides, -2 in other compounds, except with F

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on: (17)

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-1 with metals, nonmetals (besides O), and halogens lower in the group

Front 195

on: S8

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0

Front 196

on: Al2O3

Back 196

Al = +3 O= -2

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on: N2H4

Back 197

N = -2 H = +1

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on: S2(O3)2-

Back 198

S = +2 O = -2

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on: HP(O4) 2-

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H = +1 P= +5 O = -2

Front 200

on: CH3OH

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C = -2 H = +1 O = -2

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if x loses electrons…..

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x is oxidized x is the reducing agent x increases its oxidation number

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if y gains electrons….

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y is reduced y is the oxidizing agent y degreases its oxidation number

Front 203

12.19 mL of 0.1038 M KMnO4 were required to oxidize 25.00 mL of FeCl2. What is the molarity of the FeCl2, given the reaction: MnO4- (aq) + 5 Fe2+ (aq) + 8H+ (aq) ---> Mn2+ (aq) + 5Fe3+ (aq) + 4H2O (l)

Back 203

0.01276 M

Front 204

A + B ---> C

Back 204

Combination

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C ---> A + B

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Decomposition

Front 206

A + BC ---> AC + B

Back 206

displacement

Front 207

metal activity series

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Li, K, Ba, Ca, Na, Mg, Al, Mn, Zn, Cr, Fe, Cd, Co, Ni, Sn, Pb

Front 208

reversible reaction

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reaction that proceeds simultaneously in both directions

Front 209

equilibrium

Back 209

the forward reaction and the reverse reaction proceed at equal rates

Front 210

To standardize an HCl solution, 50.00 mL of HCl is put in flask with indicator. 0.1524 M NaOH goes into buret with initial reading of 0.55 mL and an end point reading of 33.87 mL. What is the concentration of the HCl solution?

Back 210

0.1016 M HCl

Front 211

Oxidation

Back 211

the LOSS of electrons (LEO)

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Reduction

Back 212

the GAIN of electrons (GER)

Front 213

combustion reactions

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2C4H10 + 13O2 ----> 8CO2 + 10H2O