Chemistry 1A Final Exam Review Sheetanswer Key

Chemistry 1A final exam review sheetAnswer Key

What is qualitative data? Descriptive data
What is quantitative data?Numerical data
What are the SI base units? Meter, kilogram, Kelvin, second, mole,
What do these SI base units measure? Distance, mass, temperature, time, amount of a substance
How does one determine the number of significant digits? Use the pacific/Atlantic
What are the steps to the scientific method?Ask question, form hypothesis, make observations, experiment, draw conclusion
What is precision?How close answers are to each other
What is accuracy? How close your value is to the accepted value
What is a physical property?Characteristic that describes a substance without changing it into something new
Give 4 examples of physical properties.Color, texture, density, size
What is a chemical property?Characteristic that describes how a substance undergoes a chemical change
Give 3 examples of chemical properties.Flammability, rusting, oxidizing, combustability
What is a physical change?Changing phase but not the chemical make up
How do you know if a physical change has occurred?Can change it back
What is a chemical change?Change that results in a new substance formed
How do you know if a chemical change has occurred?Can’t change it back
What are the six phase changes of matter? Melting, freezing, sublimation, deposition, vaporization, condensation
Define each phase change of matter. Solid,  liquid  gas
Define element.Made up of only one type of atom
Define compound. Two or more different atoms bonded chemically
Define mixture. Two or more substances that are combined in a physical way and each substance maintains its own properties.
What is the difference between a compound and a mixture?Compound is bonded chemically and a mixture is not. Mixture can be separated by physical means (filter)
What is the formula for determining the amount of energy lost or gained by a substance? Q=m∆Tc (m=mass, ∆T= Tf- ti, c= specific heat)
What does each variable stand for in the equation from #23? See above
What is the formula for density? Density = mass/volume
What are all the parts Dalton’s atomic theory? see your notes
What did Aristotle contribute to the atomic theory?4 elements-earth, air, water, and fire
What did Chadwick discover?neutrons
What did Bohr discover?Electrons orbit nucleus in specified paths
What did Democritus do?Named the atom
What did Rutherford discover?nucleus
How did Rutherford discover #31?Used gold foil
What did Thomson discover?electron
How did Thomson discover #33?cathode ray tube
What is the law of multiple proportions? See notes
What is the law of definite proportions? See notes
What is an isotope?Atoms that are the same (atomic #), but have different numbers of neutrons
How do you find the mass number? Protons + neutrons
How do you find the number of neutrons?Mass number – proton (atomic) #
List the electron configuration/noble gas configuration/orbital notation for the following elements: Mg, Ca, F, Se, Si, P, S, As
What are the four quantum numbers assigned to every electron in a neutral atom? Principal- main energy level, angular momentum – sublevel, magnetic- path electron takes around nucleus, spin- which way it spins
What do each of the four quantum numbers represent?See above
What are the four sections of the periodic table?S block, p block, d block, f block
What are the sub atomic particles of an atom?Proton +, neutron 0, electron -
What is the charge on each sub atomic particle in an atom?
Where is each sub atomic particle in the atom?P+/n0 in nucleus, E- in electron cloud
What does the proton determine?Identity of atom
What does the electron determine?Behavior of the atom
What is group 1? Alkali metals
What are some characteristics of group 1?
What is oxidation # (charge) of group 1?+1
What is group 2?Alkaline earth metals
What are some characteristics of group 2?
What is the charge on group 2?+2
What are groups 3-12 called?Transition metals
What are some characteristics of #55?
What is group 17?halogens
What are some characteristics of group 17?
What is the charge on group 17?-1
What is group 18? Noble gases
What are some characteristics of group 18?
Who added that group to the periodic table?Sir William Ramsey
What are the two sections at the bottom of the periodic table called? F-block, lanthanide/actinide series
Where are the radioactive elements located on the periodic table?actinides
What did Mendeleev do?Arranged by atomic mass
What was wrong with his organization?inconsistencies
What did Moseley do?Arranged by atomic #
What is atomic radius?
What are the group and periodic trends of atomic radius?
What is ionization energy?Energy required to remove an electron from a neutral atom
What are the group and periodic trends of ionization energy?
What is electronegativity?Ability of an atom to attract electrons
What are the group and periodic trends of electronegativity?
What is a cation?+ ion
What is an anion?- ion
What are valence electrons?
What element has the highest electronegativity?F
What are metalloids? Group of elements in the p block that have characteristics of both metals and non-metals
What is a group?Columns on the periodic table
What is a period?Horizontal rows on the periodic table
What is the law of conservation of mass?Cannot create nor destroy it, only change it.
What is a binary acid?Acid with two elements, one is H2, other is a non-metal
What is an oxyacid (ternary)? acid with more than two elements, one is H2, other is O2, and usually another non-metal
How do you name a binary acid?Prefix hydro, suffix- ic
How do you name an oxyacid?PI ends with ate  suffix ic, PI ends with ite suffix ous
What kind of substances form compounds?Metals (cations)/non-metals (anions) NO PREFIXES used
What happens with electrons with these compounds?Transfer electrons
What kind of substances form molecules?Metalloids/non-metals, non-metals/non-metals
What happens with electrons with these molecules?Share electrons
What is the difference among a nonpolar, polar, and ionic bond?0-.4 nonp, .5-1.7 polor, > 1.7- ionic
One mole of a substance equals how many? 6.022 • 1023
What are the diatomic molecules? H2, N2, O2, F2, Cl2, Br2, I2… BrINClHOF

PROBLEMS:

Fill in the chart:

Nuclear Symbol / Mass Number / Atomic Number / # Protons / # Neutrons / # Electrons
1. / / 59 / 28 / 28 / 31 / 27
2. / 35
Cl
17 / 35 / 17 / 17 / 18 / 17
3. / / 1 / 1 / 1 / 0 / 0
4. / 32
S -2
16 / 32 / 16 / 16 / 16 / 18

Give the number of significant figures:

1. 420.0 ____4_

2. 7589 ____4_

3. 432506.43 ___8__

4. 0.0000476 __3___

5. 0.03 __1___

6. 35.17 ___4__

7. 0.00004 ___1__

8. 8671.5 __5___

Express your answer to the following with the appropriate number of significant figures:

1. 2.21 x 0.3= 0.7

2. 789.234 ÷ 47.36 =16.67

3. 2.90 x 0.01733 x 920= 46

4. 2.02 x 4.113 =8.31

5. (72) (4.022) =32

9.03

Convert the following:

1. 34 m = _3400____ cm

2. .15 mg = _0.00015____ g

3. 32.98 L = _32980___ mL

4. 1286 m = _1.286____ km

5. 72 cm = _0.72____ m

6. 948 mm = _94.8__ cm

7. 32 Dm = _320___ m

8. 87 km = _870__ Hm

Place the following in scientific notation:

0.000 000 1101.1 x 10-7

0.000 0272.7 x 10-5

6 220 000 0006.22 x 109

77 000 000 000 7.7 x 10 10

410 0004.1 x 105

0.000 000 0111.1 x 10-8

Place the following in standard form:

4.3 x 108 430000000

2.5 x 10-100.00000000025

1.2 x 10-40.00012

6.2 x 1011620000000000

4.4 x 10-60.0000044

1.3 x 105130000

Execute the following calculations

( 1.10 x 103 ) ( 3.922 x 106 )4.31 x 109

( 2.377 x 106 ) (1.81 x 109 )4.30 x 1015

(6.30 x 108 ) ÷ ( 2.50 x 103 )2.52 x 105

( 7.64 x 106 ) ÷ (1.343 x 108 )5.69 x 10-2

Given that the density of iron is 11.35 g/cm3, what would be the volume of a 5.7 gram piece of iron?

V = 0.50 cm3

What is the density of 37.72 g of water whose volume is 6.80 cm3?5.55 g/cm3

The density of Aluminum is 2.70 g/cm3. The volume of a solid piece of Al is 1.50 cm3. What is the mass of this piece?4.05 cm3

NP Assmallest ionization energy

OCNhighest ionization energy

AlSiPmost electronegative

ClBrIleast electronegative

NaKLilargest atomic radius

NaMgAlsmallest atomic radius

Write the chemical formula and compound name for the following:

1) Ca and NO3 / 6) V3+ and CrO4 / 11) Al and OH / 16)Pb2+and C2H3O2
2) Ca and PO4 / 7) K and ClO3 / 12) Fe2+ and ClO3 / 17) NH4 and C2O4
3) K and SO4 / 8) Sn4+ and OH / 13)Cu+ and SO4 / 18) Na and PO4
4) Ba and NO3 / 9) Mg and NO3 / 14) K and MnO4 / 19) Cr3+ and NO3
5) Al and SO4 / 10)NH4 and SO4 / 15) Sn2+ and PO4 / 20) Pb4+ and SO4

Ca(NO3)2 Calcium nitrate
Ca3(PO4)2 Calcium phosphate
K2SO4 Potassium sulfate
Ba(NO3)2 Barium nitrate
Al2(SO4)3 Aluminum sulfate
V2(CrO4)3 Vanadium (III) chromate
KClO3 Potassium chlorate
Sn(OH)4 Tin (IV) hydroxide
Mg(NO3)2 Magnesium nitrate
(NH4)2SO4 Ammonium sulfate
Al(OH)3 Aluminum hydroxide
Fe(ClO3)2 Iron (II) chlorate
Cu2SO4 Copper (I) sulfate
KMnO4 Potassium permanganate
Sn3(PO4)2 Tin (II) phosphate
Pb(C2H3O2)2 Lead (II) acetate
(NH4)2C2O4 Ammonium oxalate
Na3PO4 Sodium phosphate
Cr(NO3)3 Chromium (III) nitrate
Pb2SO4 Lead (IV) sulfate

Name the following molecules:

CO2carbon dioxide
CCl4carbon tetrachloride
PCl5phosphorus pentachloride
SeF6Selenium hexafluoride
As2O5Diarsenicpentaoxide
SO3Sulfur trioxide
ICl3Iodine trichloride
PBr5phosphorus pentabromide

Write the formula for the following binary molecular compounds:

carbon tetrabromide CBr4
silicon dioxideSiO2
tetraphosphorusdecoxideP4O10
diarsenictrisulfideAs2S3
sulfur trioxideSO3
diphosphorus pentoxideP2O5
dinitrogen trioxideN2O3

Tell what type of bond (based on electronegativity values) exists between the following pairs of atoms:

a. H and I npd. Se and Snpg. Li and FI

b. S and Ope. C and Hnph. Cu and Sp

c. K and Br If. Ca and ClIi. I and Brnp

Draw the Lewis structure and predict the polarity for the following molecules:

a. CI4nonpolarc. BCl3nonpolar

b. Cl2Opolard. PI3 polar

Write the formula for the following acids:

Carbonic acidH2CO3

Chlorous acidHClO2

Iodic acidHIO3

Hydrobromic acidHBr

Arsenic acidH3AsO4

Hydrofluoric acidH2S

Sulfurous acidH2SO3

Hypochlorous acidHClO

Write the correct name for the following acids:

H3BO3Boric acid

H2SO4Sulfuric acid

HClO2Chlorous acid

H2SHydrosulfuric acid

H2CrO4Chromic acid

HClHydrochloric acid

H2SO3Sulfurous acid

Convert the following grams to moles

0.0486 g Cd0.0004
9.64 g Al 0.36
0.425 g S 0.013
86.9 g I 0.68
273.6 g Pb3N40.403
45.3 g PbF20.18
66.7 g O22.08
0.067 g CuO 8.4 x 10-6
.864 g Pt2C0.002
2.63 g N2 0.09

Convert the following moles to grams

0.982 mol Au 193.42
1.62 mol H2 3.27
0.774 molRb66.15
0.029 mol Fr 6.47
2.03 mol Al2(SO4)3 694.3
92.6 mol BeI2 2.4 x 104
4.32 mol Cr3P2941.5
0.079 mol KOH4.26
1.32 mol MnBr4494.39
0.062 molHCl2.26

Convert the following grams to atoms:

1. 0.62 g Co 6.3 x 1021

2. 4.9 g Cu 4.6 x 1022

3. 0.12 g Zn1.1 x 1021

Name the following compounds AND circle the ones that are soluble in water. Soluble in red

1. AgClSilver chloride

2.Na2SO4Sodium sulfate

3. NH4NO3Ammonium nitrate

4. Al(ClO4)3Aluminum perchlorate

5. Sr3(PO4)2Strontium phosphate

6. K2CrO4Potassium chromate

7. FeBr3Iron (III) bromide

Using the activity series, determine if the following reactions will occur. If they do, you must balance.

1. 3Na + AlBr3  3NaBr + Al

2. 2Li + CuSO4  Li2SO4 + Cu

3. 2Al + 3CuSO4 Al2(SO4)3 + 3Cu

4. Mg + LiNO3 Mg(NO3)2 + Li no rxn

Balance AND identify the following reactions:

1. Mg + Zn(NO3)2  Zn + Mg(NO3)2SR

2. Mg + 2AgNO3  2Ag + Mg(NO3)2SR

3. 2NH3  N2 + 3H2Decomp

4. 2MgO  2Mg + O2decomp

5. 2K + Cl2  2KClsyn

6. 4Al +3O2  2Al2O3syn

7. 2HI  H2 + I2decomp

8. 2C2H6 + 7O2  4CO2 + 6H2Ocombustion

9. 3Li2S + 2AlP  Al2S3 + 2Li3PDD

10. 2K2S + PbO2  2K2O + PbS2DD

Balance the following equations:

11. __2_ Al + __3__ CuSO4 ____ Al2(SO4)3 + __3__ Cu

12. ____ Pb(NO3)2 + __2__ NaI ____ PbI2 + __2__ NaNO3

13. __2__ CH4 + __3__ O2 ___2_ CO + __4__ H2O

14. __2__ Cu + ____ S  ____ Cu2S

15. __2__ Na + __2__ H2O  ___2_ NaOH + ____ H2

16. ____ C3H8 + ___5_ O2 __3__ CO2 + __4__ H2O

17. ____ Ca(OH)2 + __2__ HCl ____ CaCl2 + __2__ H2O

18. ___2_ Mg + ____ O2 __2__MgO

19. ____ C6H12O6 + __6__ O2 __6__ CO2 + _6___ H2O