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Chemistry

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chem vocabulary

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Chapter 6Periodic law- states that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties Group- A vertical column of elements in the periodic table; also called a family Period- A horizontal row of elements in the modern periodic table Representative element- groups of elements in the modern periodic table that are designated with an A (1A-8A) and possess a wide range of chemical and physical properties transition element ? Groups of elements in the modern periodic table that are designated with a B (1B-8B) and are further divided into transition metals and inner transition metals

Substance Identification Lab

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Lab 6-1 Catherine Puga Paradichlorobenzene has a very strong odor while potassium iodide does not. PDCB(paradichlorobenzene) is more volatile then potassium iodide. Volatile means that the molecular substance can evaporate easily and when it evaporates, it lets off a strong smell. A substances ability to evaporate depends on the strength of its bonds. Potassium iodide had ionic bonds whereas PDCB has London Dispersion Forces. LDF?s are the weakest type of intermolecular bonds; therefore, PDCB evaporates easier so it has a stronger odor.

Chemistry Terms

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Chemistry Chapter 8 and 9 Terms Chapter 8 Axial: in the trigonal bipyrimidal electron-pair geometry, the two positions directly across from each other. Bent: the molecular geometry of a triatomic molecule or ion in which the bond angle is less than 180 degrees. Bond Angle: the angle formed between two bond axes. Bond Axis: an imaginary line connecting the nuclei of two bonded atoms. Bond Length: the distance between the nuclei of two bonded atoms. Bond Order: the number of bonding electron pairs shared by two atoms in a molecule or polyatomic ion. Bonding Pair: a pair of electrons that is shared between two atoms. Bonding: describes the forces that hold adjacent atoms together. Chemical Bond: an attractive force between two atoms that causes the atoms to be attached together.

Basic Organic Chem

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/ \ \.1- 2\-\ -c-c.-S-t-I I M H n '10) ~\ - L.-C-D"I-It" H H -I - \ I \ ,,' " '--------------------'-...-/;- H-C-C.-.~-.~-~~~-t-l ++\ ~ SulE1..x'S stv-Y\ -fL;---- H ~ ok;" C\C.icJ w bCAs.e.'""l. ' G t-l Wr12:l + +-I 0 ~ G H ~H~_-_4_+l..??e_T" _ bo~\ j( c .,..i 1-.)\-1 + -4-1 0 ~ l-.)+I T \ 61-\- w .,.~""....0----.------ _____ - """??.?..,OY:. -,~----- ~,,----- ."."" 1 e-..,-,,--r.,., _____ c:r~ .1-- 4 -_-lrt-,.>-t-_ ..???_- -4-t-'*-_-- __ - ---- +I- e' - (- 's - \-\ t1 - c. -c.- \-~ +t~c\.;.~-o -+-I -1-\ ~ h fl c. ...h :, Y,'fJ~~-/1 - Thlol oJ.e".eSI'''.'\-- _ .. -----------

Basic Organic Chem

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/ \ \.1- 2\-\ -c-c.-S-t-I I M H n '10) ~\ - L.-C-D"I-It" H H -I - \ I \ ,,' " '--------------------'-...-/;- H-C-C.-.~-.~-~~~-t-l ++\ ~ SulE1..x'S stv-Y\ -fL;---- H ~ ok;" C\C.icJ w bCAs.e.'""l. ' G t-l Wr12:l + +-I 0 ~ G H ~H~_-_4_+l..??e_T" _ bo~\ j( c .,..i 1-.)\-1 + -4-1 0 ~ l-.)+I T \ 61-\- w .,.~""....0----.------ _____ - """??.?..,OY:. -,~----- ~,,----- ."."" 1 e-..,-,,--r.,., _____ c:r~ .1-- 4 -_-lrt-,.>-t-_ ..???_- -4-t-'*-_-- __ - ---- +I- e' - (- 's - \-\ t1 - c. -c.- \-~ +t~c\.;.~-o -+-I -1-\ ~ h fl c. ...h :, Y,'fJ~~-/1 - Thlol oJ.e".eSI'''.'\-- _ .. -----------

Solubility Chart

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Solubility Guidelines for Common Ionic Compounds in Water Soluble Compounds Important Exceptions Compounds containing the following: NO3- None C2H3O2- None Cl- Compounds of Ag+, Hg22+, Pb2+ Br- Compounds of Ag+, Hg22+, Pb2+ I- Compounds of Ag+, Hg22+, Pb2+ So42- Compounds of Sr2+, Ba2+, Hg22+, Pb2+ Insoluble Compounds Important Exceptions Compounds containing the following: S2 Compounds of NH4+, the alkali metal cations, and Ca2+, Sr2+, and Ba2+ CO32- Compounds of NH4+, the alkali metal cations PO42- Compounds of NH4+, the alkali metal cations OH- Compounds of the alkali metal cations, and Ca2+, Sr2+, and Ba2+ Common Strong Acids and Bases Strong Acids Strong Bases Hydrochloric, HCl

Compound Naming and Molecular and Empirical Formulas

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Compound Naming Ionic: ends in ?ide NaCl -binary compound (two element) - a ratioempirical formula - sodium chlorineide Metals: use roman numbers to indicate charge What happens when you are naming metals? -Metals can take on a number of charges, and thus don?t have a set charge. For example: Cr+3Cl3- and Cr+2Cl2 both would be called ?chromium chloride? if we use the above rule. Thus, we resort to using roman numerals to denote charge. Cr+2Cl2 is now known as chromium III chloride Cr+3Cl3- is now known as chromium II chloride. Molecular: denote subscripts make sure the molecule doesn?t consist of ionic or metallic bonds CO carbon MONoxide CO2 carbon DIoxide P2S5 DIphosphorus PENTsulfide NOTE: put cations (positive) first Emperical Formula: reduce the numbers C1H2O1=CH2O

Compound Naming and Molecular and Empirical Formulas

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Compound Naming Ionic: ends in ?ide NaCl -binary compound (two element) - a ratioempirical formula - sodium chlorineide Metals: use roman numbers to indicate charge What happens when you are naming metals? -Metals can take on a number of charges, and thus don?t have a set charge. For example: Cr+3Cl3- and Cr+2Cl2 both would be called ?chromium chloride? if we use the above rule. Thus, we resort to using roman numerals to denote charge. Cr+2Cl2 is now known as chromium III chloride Cr+3Cl3- is now known as chromium II chloride. Molecular: denote subscripts make sure the molecule doesn?t consist of ionic or metallic bonds CO carbon MONoxide CO2 carbon DIoxide P2S5 DIphosphorus PENTsulfide NOTE: put cations (positive) first Emperical Formula: reduce the numbers C1H2O1=CH2O

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