Download Day 1 after school REVIEW

Day 1 after school REVIEW
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Chapters 1-4
Chapter 1 Intro to Chemistry:
Scientific Method: systematic approach, organized process used in scientific study
Qualitative:
Quantitative:
Independent variable:
Dependent variable:
Control:
Theory: explanation of natural phenomena based on observations and investigations
over time.
Law: a relationship in nature that is supported by many experiments.
Lab Safety
Lab Equipment
Chapter 2 Analyzing Data
1. Convert the following temperatures:
a. 50◦C =_____K
b. 265K = _____◦C
2. 1 mL = 1cc = 1g
a) Calculate the volume of a 4.5g sample of Tin using the following image.
3. Place the following in scientific notation:
a. 1,392,000
b. 0.000028
4. Express the following as a normal numeral:
a. 4.87 X 10-3
b. 3.54 X 105
5. Solve the problem:
(4 X 102) X (1 X 108) =
6. Perform the following conversions using conversion factors:
a. 360 s = _________ms
b. 4800g = ________kg
7. The accepted density for copper is 8.96g/mL. Calculate the percent error if a
student observes it to be 8.92g/mL. Show formula, work and answer.
8. Sig Fig Rules:
1.
2.
3.
4.
a) Determine the number of sig figs in each of the following:
a. 0.049450
b. 1.0200 X 105
c. 0.00084
b) Math with Sig Figs:
+/Least places after decimal and
use sig figs in that number
258.3 + 257.11 + 253 =
9) Graphing Data:
X/division
Least sig figs
120 X 0.10 =
Chapter 3 Matter Properties and Changes
Solid
Def shape and volume
Liquid
flows, constant volume,
takes shape of container
Gas
flows to fill container,
fills entire volume
3 molecules of Bromine @ STP
5 molecules of water
vapor
Draw the following:
7 molecules of Iodine @
STP
Physical Property:
Chemical property:
Physical change:
Chemical change:
Evidence:
1.
2.
3.
4.
Physical methods of separation:
1. Filtration:
2. Distillation:
3. Crystallization
4. Chromotography
Chapter 4 The Structure of the Atom
1. History:
1) Democritus - Greek philosopher
matter is composed of tiny particles called atoms which could not be subdivided or made
any smaller
2) John Dalton
a) matter is composed of tiny particles called atoms
b) atoms of a particular element are alike in size, shape, and weight but differ from atoms
of other elements
c) during chemical changes, atoms of different elements unite forming molecules
(compounds)
d) during these chemical changes, atoms themselves do not change, that is, are not broken
down
e) when atoms combine, they do so in definite whole number ratios by weight
3) J. J. Thomson - gas tube experiments of the late 1800's
a) when a high electrical voltage was placed across electrodes in a glass vessel from
which most of the air had been removed an electrical
discharge occurred
b) from the direction of deflection the charge on these particles had to be negative
c) in 1897 J. J. Thomson first measured the ratio of charge to mass, e/m, of these small
mass,
negatively charged, high velocity particles called electrons “plum pudding model”
4) Rutherford-Geiger-Marsden gold foil experiments - 1911
a) these men knew that alpha particles were, charged helium ions that traveled in straight
lines at very high speeds
b) the plum pudding model of the atom (J. J. Thomson - 1897) said atom was sphere of
positive matter in which electrons were randomly
embedded (like raisins)
c) according to the plum pudding model the expected results of shooting a beam of alpha
particles at thin gold foil should be that the alpha particles
would pass straight through since there would be
no concentration of charge and mass large enough to deflect the relatively massive alpha
particle
d) actual results: most of the particles passed through unharmed (missed Au atoms) a few
were
deflected off to the side a very few were reflected backward (head on collision with
nucleus
e) initial conclusions reached:
1) scattering must be due to encounters with charged atomic particles that are much
smaller than
the atom and at least as heavy as an alpha particle
2) must be some positive electric charges inside the atom to compensate for negative
charges of the electrons
3) must be something in the atom much heavier than an electron to account for the mass
of the atom
4) atoms must be mostly empty space
f) final conclusions:
1) positively charged protons concentrated in region inside atom called nucleus
2) atoms total diameter much larger than that of the nucleus
3) negatively charged particles, called electrons, were circling in orbit around the
nucleus (a
4) the positive electrical charge of the proton is equal in strength to the negative
electrical charge
of the electron
5) the weight of the proton is 1836 times as great as the weight of an electron
6) a particle in the nucleus having no electrical charge was predicted
5) James Chadwick - 1932
Found neutron
2. Modern Atom:
What is atomic number?
What is mass number?
12.011
C
6
What is an isotope?
What is an ion?
3. Fill in the following table:
Notation
Atomic #
Mass #
15
32
119
Protons
Electrons
neutrons
24
51
22
48
30
charge
-3
4. Three magnesium isotopes have atomic masses and relative abundances of
23.985amu(78.99%), 24.986amu(10.00%), and 25.982(11.01%). Calculate
the average atomic mass. Show formula, work and answer with units.
5. Complete the following equations:
a. 222Rn
b.
90Sr
c.
37Ca