FINAL REVIEW

PRE AP/ GT CHEMISTRY
MRS DAVIS
1. Steps of the scientific method
a. Observation
b. Problem
c. Experiment
d. Data
e. Analysis
f. Conclusion
g. Application
2. A theory can be disproved and a law has been proven
3. Physical properties are color, size, shape, hardness, mass, melting point, boiling point
a. Chemical properties include explosiveness, fermentation, rusting
4. Physical changes include evaporation, freezing, melting, cutting
a. Chemical changes include fermentation, corrosion,burning
5.
1,567,900,00 = 1.567x109 .0006890012= 6.89x10-4
6. Accuracy is the closeness of a measurement to its true value, Precision is the ability to get the
same measurement multiple times
7. Democritus was the first to suggest the existence of atoms
a. Thomson used cathode rays to discover electrons because gases in a cathode ray are only
electrons
b. Rutherford’s model of the atom explained that the region outside the nucleus is mostly empty
space in which the electrons are
c. Dalton’s model of the atom explained what an atom was
d. p 108 #3 Dalton actually tested his experiment
e. p 112 #6Thomson used the cathode ray tube to prove that an electron was negative
f. p 121
i. #19 The atomic number tells how many protons and electrons are in an element, atomic
mass is a combination of protons and neutrons
ii. #23
a. a
b. b
c. c
8. Some properties of metal include: luster, conduct electricity, malleability, ductility
a. nonmetals are non-lustrous, poor conductors of electricity
9. p 129
a. #34
i. a. A beam of electrons is deflected by an electric field toward the positively charged plate.
ii. b. Cathode rays were always composed of electrons regardless of the metal used in the
cathode ray
#39
The atomic number has equal numbers of protons and neutrons
#42
Atomic #
Mass #
# protons
# neutrons
# electrons
Symbol
9
19
9
10
9
F
14
29
14
15
14
Si
22
47
22
25
22
Ti
25
55
25
30
25
Mn
10.
a.
Cations are positively charged ions- Anions are negatively charged ions.
p 137
i.
4. Metals are cations and nonmetals anions
ii.
5.-ide at the end of an ion tells you that it is an anion
iii.
8. K+, Zn2+
iv.
9. a. flouride ion F- , sulfide ion S2-
11. Metallic cations and nonmetal anions form ionic compounds
12. Molecular formulas show the number and kinds of atoms in a molecule of a compound
a. 142 #12 A chemical formula shows the kinds and numbers of a toms in the smallest rep unit
of the substance. The molecular formula shows the number of each kind of atom in a
molecule of a compound. The formula unit shows the lowest whole-number ration of ions
in a compound.
13. Ionic Charges
a. p 148
i. 20. Look at the group the element is found in
ii. 21. Polyatomic ions contain two or more tightly bound atoms that behave as a unit.
iii. 22. a. potassium K+ b. sulfide S2- c. no ion d bromide Br- e. beryllium Be2+ ,sodium
Na+
iv.
23. a NH4+ b. Sn2+ c CrO42- d. NO3- e CN- f. Fe3+
14. Writing formulas for ionic compounds
a. p 156
i. 32 The formula must be written so the net ionic charge is zero. The cation is written
first, the anion is written second. To write the name from the formula, name the cation
followed by the anion.
ii. 33. Write the formula (symbol and charge) for each ion. Then use the crisscross method.
To do the reverse, name the cation followed by the anion.
iii. 34.
a. Cr3+ NO2- Cr(NO2)3
1.
2. b. Magnesium phosphate
3. c. Lithium Flouride
d. Na+ ClO4- NaClO4
4.
5. e. Lead II Acetate
6. f. Mg2+ HCO3- Mg(HCO3)2
iv. 35. Parenthesis are used when more than one polyatomic ion is needed to balance a
formula.
15. Moles and Mass
a. p 181
i. 11. One mole of any substance contains Avogadro’s number (6.02x1023) of
representative particles
ii. 12. Gram formula mass
1. a. 2 Li + S 2*6.94 + 32.07= 45.9 g
2. b. Fe+ 3 CL 55.85+ 3*35.45=162.3 g
3. c. Ca + 2*O+2*H 40.1+2*16+2*1.01= 74.1g
iii. 13. a 3 b. 4 c.3 d.9
iv. 14. Moles of the following a. 1.5 x1023/6.02 x1023=.249 moles b. 1x109/6.02 x1023
=1.66x10-15 moles c. 6.02 x1022 /6.02 x1023 = .1 moles d. 4.81 x1024 /6.02 x1023
=7.99moles
16.The diatomic seven are hydrogen, oxygen, chlorine, bromine, nitrogen, fluorine and iodine
17. p 189
29 a 9.03+ 3.48= 12.51 %Mg 9.03/12.51*100= 72% %N 3.48/12.51*100= 28%
b. %Ag 29/33.3=87% %S 4.3/33=13%
18. p 211
9. a CuS + O2 Cu + SO2
b. H2 + O2 H2O
c. NaHCO3NaCO3 + CO2 + H2O
10.a. 2,1,2 b. 1,3,2,3 c. 4,5,1 d. 2,1,2
11. SO3 b. KN O3 c. d. Cu e. Hg(l)
12. The number and kinds of atoms in the reactants are equal to those of the products.
19. Combination- two things combine to make one
Decomposition- one thing breaks down to make two
Single-replacement- one element replaces a second element in a compound
Double replacement- an exchange of positive ions between two reacting compounds
Combustion- an element or compounds reacts with oxygen producing carbon dioxide and
water
20. Activity series of metals lists metals in order of decreasing reactivity and it tells whether one
metal will displace another metal from a compound.
21. Bohr’s model of the atom said that electrons orbit the protons which are in the center of the
nucleus with the neutrons.
22.1st energy level=2
2nd energy level=8
3rd energy level=18
23. a Aufbau principle- electrons enter orbital’s of lowest energy first.
b. Pauli exclusion principle an atomic orbital may describe at most two electrons
c. Hund’s rule- When electrons occupy orbital of equal energy, one electron enters each orbital
until all the orbital’s contain one electron with parallel spins
24- Take a break!!!
25. Li 1s22s1
F 1s22s22p5
Rb [Kr] 5s1
26. The noble gases all end with full s and p orbital’s equaling 8 electrons in their outer shells
27. p 406
6. a,c
7. sodium. Aluminum.sulfur.chlorine,:periodic trend
8. The anion is larger than its atom
9. a. sodium, b phosphorus
10.noble gases: group 0, representative elements: groups 1a-7a: transition elements 1b-8b:
inner transition elements a separate section between Groups 2a and 3b
11.a B 1s22s22p1
b. Mg 1s22s22p63s2
c. As [Ar]4s24p3
12. Na, Mg,Cl
28. Ba [Xe]
29. p 418
1. The group number equals the number of valence electrons for representative elements
2. It is easier for a metal to lose electrons and for a nonmetal to gain electrons to achieve the
electron configurations of a noble gas.
3. a. 1 b. 4 c.2 d. 6
4. a. K b. C c. Mg d O
5. Cu+[Ar]3d10
Cd 2+ [Kr]4d10
6. a lose 2, b gain 1, c. lose 3, d. gain 2
30. p 425
9. attraction between oppositely charges ions formed through electron transfer
10. Ionic compounds conduct electricity when melted and in aqueous solution because their
ions are free to move about
11. a K2S b. Cao c. Na2SO4 d. AlPO4
12. a KNO3 b. BaCL2 c. MgSO4 d. Li2O e. (NH4)2 CO3 f. Ca3 (PO4)2
31. p 429 #15 The sea of free-flowing electrons conduct electricity and heat.
32 Why do elements bond covalently? So that both can attain a noble gas formation
33. Please look at lewis diagram notes
34. The VSEPR theory is the valence shell electron pair repulsion theory and states that because
electron pairs repel, molecular shape adjusts so the valence electron pairs are as far apart as possible.