Chemistry Review- Fall Final 2011
Name: ______
Due Date: ______
Chapter 1: pg. 2
Chemistry is the study of ______
Define the following terms and give an example of each:
matter
What is difference between mass and weight?
Define Scientific Method
Compare the following and give an example of each:
qualitative data & quantitative data
hypothesis & theory
Know your Lab Safety Rules: pg. 16 - some examples may include:
What are the correct steps for:
Lighting a burner?
Heating liquid in a test tube?
Diluting an acid?
Detecting an odor?
What is the correct procedure to prevent chemical spills & to clean them up if necessary?
What is the correct way to dress for lab?
Chapter 2: pg. 24 Define the following terms and give examples of each:
Name the standard SI units
list 3 other common units we use that are NOT SI
metric prefixes (Table 2-2, pg. 26)
gosh man, Kenya does contain many mangy nutria pets!
Other ways of expressing 25.3 cm = ______mm = ______m = ______nm = ______km
Convert 10.0 km to meters ______m
4.75 mg to grams ______g
significant figures: rules for rounding
Round these to 3 sig figs: 45678000 à ______2.344 x 10 5 à ______
scientific notation (1 digit to left of decimal)
p32 #12 & 13
mass is ______and is measured with______
volume is ______
how measured when irregularly shaped?
What is the volume of a marble if it is dropped into 25.0 ml of water and causes the water level to rise to 27.3ml ?
density =
ex: p29 #1 & 3
What is the difference between accuracy and precision?
Chapter 3: pg. 54 Define the following and give examples of each:
element vs. compound vs. mixture What are each of these? H, H2O, Ni, NO, salt water, cement, brass, copper
given an example of a heterogeneous mixture ______a homogeneous mixture ______
conservation of mass p65 # 6 & 7
% composition problem p76 # 20-22
Compare and give examples of the following:
physical & chemical properties p82 #37
the 3 states of matter
physical change vs chemical change
give examples of each p82 #39
is a change of state physical or chemical?
Chapter 4: pg. 86 Define the following:
atom (no charge) smallest particle of an element that has ______
how does it differ from ion?
nucleus
electron
How does the mass of an electron compare to that of a proton or a neutron? (mass chart p97)
proton (# of p+ same as ______)
p 99 #11-13
neutron
isotope
ex:p 101 #14
Dalton’s atomic theory
Thomson’s plum pudding model
Rutherford’s nuclear model (p94)
The gold foil experiment showed what?
Atomic Number
Atomic Mass vs Mass Number
average atomic mass à weighted average based on what 2 things ?
p 104 #15 & 17
Ch 25 - Nuclear Chemistry
1. The three major types of naturally occurring radiation are ______.
2. An alpha particle contains two protons and two neutrons, and has a______charge.
3. An alpha particle is equivalent to a ______nucleus.
4. The alpha particle is represented by _____ or ______.
5. A ______shows the atomic # and mass # of the particles involved.
6. Beta particles consist of fast moving electrons with a _____ charge.
7. Beta particles are represented by the symbol _____.
8. Gamma rays are high-energy radiation that possesses no ______or ______.
9. Gamma rays are represented by the symbol _____.
10. The conversion of an atom of one element to an atom of another element is called______.
11. Elements with atomic numbers greater than 93 are known as ______elements.
12. A ______is the time required for one-half of a radioisotope’s nuclei to decay
13. The splitting of a nucleus into fragments is known as nuclear ______and is
accompanied by a very large release of ______.
14. The combining of atomic nuclei with a very large release of energy is nuclear ______.
Problems
Complete the following nuclear equations and state the type of nuclear decay.
15. ______
16. ______
17. ______
18. ______
19. ______
20. ______
Half-Lives
154. If gallium-68 has a half-life of 59.2 minutes, how much of a 30mg sample is left after three half-lives?
155. If the passing of five half-lives leaves 50.0mg of a strontium-90 sample, how much was present in the beginning?
Chapter 5: pg. 116 Define and understand the following:
electromagnetic radiation (EMR)
wavelength
frequency
amplitude
photon
ground state
excited state
atomic orbital
Is it the exact path or is it the probable location of an electron?
energy levels
electron configuration (hint: add the exponents to = at. #)
p 139 #18-22
The halogen family would have an e- configuration ending with what?
Alkaline earth metals e- config ends with?
Transition metals e- config ends with?
noble gas configuration notation
What is wrong with these notations: Zr = [Kr] 5s25d2 Ga = [Ar]4s23d11 Ne = 1s22s22p10
p 147 # 80
Lewis dot diagram
p 141 # 23
valence electrons are those in the ______shell. All elements in the same ______have the same # valence e-
p175 # 66
Octet Rule
Chapter 6: pg. 150 and Chapter 7: pg. 178
Define: Periodic Law
What is an ion?
How is it different from an atom?
Periodic Trends: be able to compare 2 elements using a periodic table for these characteristics:
atomic radius, p175 # 65
ionic radius,
electronegativity (down a group & across a period) p 175 # 69
Describe the properties of the following and know where they are located on the Periodic Table:
Groups vs. Periods
A vertical column is a ______or ______. A horizontal row is a ______
elements in families (groups) tend to act alike b/c ______
p 175 # 68
representative elements – (which groups?)
transition elements – (which block?)
actinides
lanthanides
halogens
of these: F, Cl, Br, I which has strongest attraction for e- & is most reactive?
alkali metals
characteristics:
tend to react w/ ______b/c have 1 valence e- and ______want 1 e-
which alkali metal would be most reactive around halogens? Why?
alkaline earth metals
tend to have what charge? why?
which one in this family gives up its valence electrons the easiest and is most reactive?
noble gases
Why do they act the way they do?
Can they bond?
metals vs nonmetals
s,p,d,f, blocks
p 162 #7-9,
p 174-5 #45, 70
What is electronegativity?
Chapter 8: pg. 210 and Chapter 9: pg. 240
Define the following and give examples of each:
chemical bond
cation
anion
polyatomic ion
Define and compare the 3 types of chemical bonds, and give examples of each:
1) ionic (salt)
2) covalent (molecule)
3) metallic (alloy)
How are ionic compounds named?
When do you use Roman numerals?
How are covalent compounds named?
Know the prefixes for 1-10
Draw the Lewis Dot Structures for the following and label any lone pairs of electrons. Name the shape.
NH3 CCl4
CH4 H2O
How many electrons are shared in each?
single bond double bond triple bond
Write the correct name or formula for ionic cmpds and molecular cmpds and acids:
Do p 236 # 60,
74,
75,
76,
79,
88
And p 272 # 94
95
96
97
98
128
List the seven elements which are diatomic.
Chapter 10: pg. 276 Define the following:
reactant
product
subscripts
coefficients
aqueous solution
precipitate
catalyst
How do you signify these last 3 when writing an equation?
4Al + 3O2 à 2Al2O3
How many molecules of aluminum react with 3 molecules of oxygen in this equation?
How many molecules of aluminum oxide are produced?
How many atoms of Al are on each side? How many atoms of oxygen are on each side?
A balanced equation has the same # and types of atoms on both sides à law of ______of ______
Be able to write and balance equations: p304 # 71-79
Be able to identify the type of reaction p 304 # 80-84
synthesis reaction (also called composition)
decomposition reaction
single replacement reaction
double replacement reaction
acid + base à
combustion reaction
what is a major physical indicator of this type of reaction?
Given the reactants, be able to predict the products. p 304 #85,87,88,89
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