electron shells
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Electron shells: 1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p Stoichiometry / molar mass X 6.022 x 1023 Grams Moles A Atoms X molar mass / 6.022 x 1023 X Mole Ratio / molar mass X 6.022 x 1023 Grams Moles B Atoms ----- X molar mass / 6.022 x 1023
Gas stoichiometry / molar mass X 22.4 Grams Moles A Liters @ STP X molar mass / 22.4 X Mole Ratio / molar mass X 22.4 -Grams Moles B Liters @ STP X molar mass / 22.4 Balancing Redox
1) Bring down target element with compound (oxidation half-reaction first.)2) Balance target elements.3) Balance other elements (except O & H.)4) Balance oxygen by adding H2O.5) Balance hydrogen by adding H+.6) Make any net charges balance using electrons.7) When both half reactions are balanced combine them by multiplying by the lowest
common multiple. pH - log
[OH-] pOH antilog 10 -14 14 # # - log [H3O+] pH antilog SolutionsMolarity: M = moles / LTitrations: M1V1 = M2V2
Gas LawsCombined Gas Law: P1V1 / T1 = P2V2 / T2
Ideal Gas Law: PV = nRT
Variable Quantity UnitsP Pressure AtmV Volume LT Temp KR Constant 0.0821
L atm mol K
n Moles moles ThermodynamicsSpecific heat: q = (cp)(m)(∆t) Free Energy: ∆G = ∆H – T∆S
Variable Quantity Unitsq Heat Jcp Specific
heatJ/(g K)
m Mass G∆t Temp K or 0C∆G Free
energykJ/mol
∆H Enthalpy kJ/molT Temp K∆S Entropy kJ/mol
ElectrochemistryE0
cell = E0cathode – E0
anode
Ch. 1 Worksheet
1. Classify each of the following as a homogenous or heterogeneous substance.
a. _______________ Soda pop
b. _______________ Salt
c. _______________ Salt water
d. _______________ Desk
e. _______________ Raisin Bran © Cereal
f. _______________ Gold
g. _______________ Air
2. Classify each of the following as a physical or chemical change.
a. _______________ Ice melting
b. _______________ Paper burning
c. _______________ Metal rusting
d. _______________ Gas under pressure
e. _______________ Liquid evaporating
f. _______________ Food digesting
3. Why is the decomposition of mercury (II) oxide into liquid mercury and oxygen gas a chemical change and not a physical one?
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4. Draw a diagram that compares the arrangement of atoms in a solid, liquid, and gas.
5. How is energy involved in chemical and physical changes?
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6.
M
_____ Amount of matter an object has A. Homogeneous Mixture
_____ Substance made from two or more elements that are chemically bonded
B. Mass
_____ Mixture that is not uniform C. Physical Property _____ Mixture that is uniform in composition D. Matter
_____ Can be observed without permanently changing the substance
E. Heterogeneous Mixture
_____ Anything that has mass and takes up space
F. Chemical Property
_____ Smallest unit of an element G. Atom
Solid Solid
Liquid Gas
H. Compound_____ Cannot be observed without
7. A horizontal row of elements in the periodic table is called a(n) _______________
permanently altering the substance8. The symbol for the element in Period 2, Group 13 is ________________
9. Elements that are good conductors of electricity and heat are _________________
10. Elements that are poor conductors of heat and electricity are _________________
11. A vertical row of elements in the periodic table is called a(n) ________________
12. The ability of a substance to be pulled into thin wires is called _______________
13. An element that is soft and silver colored is most likely a _________________
14. The noble gases are found in which group _______________
15. At room temperature, most metals are ________________
16. Name three characteristics of non-metals
a. _______________________________
b. _______________________________
c. _______________________________
17. Name three traits of metals
a. _______________________________
b. _______________________________
c. _______________________________
18. Name three traits of metalloids
a. _______________________________
b. _______________________________
c. _______________________________
19. Name two characteristics of noble gases
a. _______________________________
b. _______________________________
20. You produce a device that requires fluorine, atomic symbol F, to function. If you were unable to find fluorine, which element would be the best replacement?
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21. What do elements of the same group in the periodic table have in common?
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22. What do elements in the same period have in common?
Unit Conversions, Scientific Notation, Percent Error
Convert the following to scientific notation
1. 65,700 __________
9. 0.0000654 __________
2. 0.008 __________
10. 19.8 __________
3. 42 __________
11. 0.0094 __________
4. 0.7 __________
12. 327 __________
5. 32100 __________
13. 0.228 __________
6. 1066 __________
14. 314 __________
7. 0.722 __________
15. 0.0224 __________
8. 87992 __________
16. 1239 __________
Convert the following from scientific notation to expanded form
17. 2.34 x 103 ____________
20. 8.1 x 102 ____________
18. 3.2 x 10-2 ____________
21. 7.6 x 105 ____________
19. 6.43 x 106 ____________
22. 1.8 x 10-4 ____________
Make the following metric conversions. Where necessary put your answer in scientific notation.
23. 4.3 liters = ____________ milliliters
24. 678 millimeters = ____________ meters 25. 9.0 centigrams = ____________ grams 26. 277 kilograms = ____________ grams 27. 11.7 grams = ____________ kilograms
Complete the following percent error calculations.
28. Experimental Value: 45 _________________ Accepted Value: 50
29. Experimental Value: 500 _________________
Accepted Value: 457
30. Experimental Value: 13 _________________ Accepted Value: 14
31. Experimental Value: 19.0 _________________
Accepted Value: 22.4
32. Experimental Value: 8.56 _________________ Accepted Value: 9.81
Significant Figures Work Sheet State how many significant figures are in each number 1) 22.200 g __________
2) 657 m __________
3) 0.000711 kg __________
4) 876.223 mg __________
5) 52.345 g __________
6) 0.3609 mL __________
7) 500000 m __________
8) 86000. mg __________
9) 8955.0 g __________
10) 87200 mL __________
Solve each problem. State your answer in the proper number of significant figures.
11) 1.0 + 13.45 __________
12) 9.2 - 5 __________
13) 5.800 + 0.4289 __________
14) 5.3 – 2.104 __________
15) 123.45 + 0.82 __________
16) 37.0 / 4 __________
17) 0.63 X 9.754 __________
18) 40.0 / 8.74 __________
19) 0.02384 X 1.37 __________
20) 2.2 X 7.776 __________
Atomic Structure Worksheet
Fill in the blanks in the following worksheet. Please keep in mind that the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table.
Atomic symbol
Atomic number
Protons Neutrons Electrons Atomic mass
C 8 12 24 31 40 40 89 30 35 42 98
W 183 105 71 95 243
Cr 27 83 209 90 142
Md 259Se 80 40 91
Molar Mass WorksheetCalculate the molar mass of the following chemicals:1) Br2
2) CsOH 3) BaCl2
4) FeF3
5) AlCl3
6) SiCl2F2
7) Mg3(PO4)2
8) SO3
9) HNO3
10) UF6
11) (NH4)2CO3
12) Al2O3
13) Pb(CH3COO)2
14) Ga2(CrO4)3
Grams/Moles Calculations
Given the following, find the number of moles: 1) 25 grams of H3PO4
Moles: __________2) 47 grams of HF Moles: ___________3) 124 grams of NaHCO3
Moles: ___________4) 0.25 grams of FeCl3
Moles: ___________5) 856 grams of Ra(OH)2
Moles: ___________6) 454 grams of copper Moles: ___________7) 28.3 grams of CO2
Moles: ____________8) 94 grams of Pb(CH3COO)4
Moles: _____________
Given the following, find the number of grams: 9) 8.4 moles of Cu(CN)2
Grams: __________10) 7.3 moles of C6H6
Grams: __________11) 17.4 moles of BaCO3
Grams: __________12) 3.9 moles of (NH4)3PO3
Grams: __________13) 8.5 x 10-2 moles of SnO Grams: __________14) 8.9 moles of ZnO Grams: ___________15) 2.8 moles of K2SO4
Grams: ___________16) 93.5 moles of NI3
Grams: __________
Grams, Molecules, and Moles Worksheet
1) How many molecules are there in 32 grams of FeF3?
Molecules: __________ 2) How many molecules are there in 250 grams of Na2SO4?
Molecules: __________ 3) How many grams are there in 4.6 x 1024 atoms of silver? Grams: ____________ 4) How many grams are there in 4.7 x 1023 molecules of AgNO3?
Grams: ____________
5) How many grams are there in 5.7 x 1023 molecules of H2SO4?
Grams: ____________ 6) How many molecules are there in 221 grams of Cu(NO3)2?
Molecules: __________ 7) How many grams are there in 4.9 x 1025 molecules of H2?
Molecules: __________ 8) How many molecules are there 230 grams of CoCl2?
Molecules: ___________ 9) How many molecules are there in 3.2 grams of NH4SO2?
Molecules: ___________ 10) How many grams are there in 4.4 x 1023 molecules of N2I6?
Grams: _____________ 11) How many molecules are there in 120 grams of CCl4?
Molecules: ___________ 12) How many grams are there in 2.3 x 1024 molecules of BCl3?
Grams: ______________ 13) How many grams are there in 5.4 x 1022 molecules of Ba(NO2)2?
Grams: _____________ 14) How many molecules are there 4.39 grams of LiCl? Molecules: ____________ 15) How many grams do 3.4 x 1021 molecules of UF6 weigh?
Grams: ______________ 16) How many molecules are there in 320 grams of NH4OH?
Molecules: ____________
Electron Configuration Practice WorksheetWrite the electron configurations using arrows of the following elements: 1) Magnesium
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2) Cobalt
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3) Krypton
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4) Beryllium
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5) Scandium
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Write the electron configurations of the following elements: 6) Nickel
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7) Cadmium
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8) Selenium
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9) Strontium
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10) Lithium ______________________________________________________
Determine what elements are denoted by the following electron configurations:
11) 1s22s22p63s23p5 ____________________
12) 1s22s22p63s23p64s23d104p65s2 _____________________
13) [Kr] 5s24d105p4 ___________________
14) [Xe] 6s24f145d7 ___________________
15) [Rn] 7s25f12 ___________________
Determine whether the following electron configurations are or are not valid:
16) 1s22s22p63s23p64s24d104p6 __________________
17) 1s22s22p63s33d6 _________________
18) [Rn] 7s25f9 __________________
19) [Xe] __________________
20) [Ne] 3p5 3s2 __________________
Chapter 4 Review SHORT ANSWER Answer the following questions in the space provided. 1. Compare and contrast Hund’s rule with the Pauli exclusion principle. ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ Write the electron configuration and orbital notation for each of the following Atoms.
3. Silicon 4. Carbon 5. Argon 6. Magnessium 7. Bromine 8. Beryllium 9. Explain what is wrong with the following electron configurations? a. ↑↓ ↑↓ ↑↑ ↑ __ ↑ __ 1s 2s 2px 2py 2pz _________________________________________________________________
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b. ↑↓ ↑↓ ↑↓ ____ ____ 1s 2s 2px 2py 2pz
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10. What do each of the quantum numbers describe:
Principal: _________________________________________________________
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Angular Momentum: ________________________________________________
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Magnetic: _________________________________________________________
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Spin: _____________________________________________________________
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