Download Chp 1,2 rev

Chp 1,2 rev.
Name:
What is matter?
Explain physical changes and properties.
How are chemical properties different? Give some examples of chemical changes.
What are periods? Groups/Families?
Give the three types of elements and their location on the periodic table.
Why are noble gases special?
What is a model?
Why do we use the SI system for measurements?
Give the base units for length, mass, volume, time, and temperature.
Convert 75 g to Kg
Convert 680 ms to Ks
What is 1 cm3 equal to ?
What is density?
How many grams are in 100ml of a solution with a density of 2.5g/ml?
Describe Solids, Liquids, and Gases.
Calculate the volume of 15 g of a solid with density of 6g/ml.
Explain precision and accuracy.
What are significant figures?
How many significant figures are in the following
103
0.0033
13.5
4500
What do you keep track of when you add/subtract measurements?
What about when you multiply/divide?
Do the following problems using correct significant figures.
3.2 x 4 =
45.67 + 7.3 =
Describe scientific notation?
Convert the following into scientific notation
45000000
0.0000313
What do direct and inverse proportional mean?
Chp 3,4 Review
Explain the laws of definite and multiple proportions.
Give Dalton’s atomic theory.
What particle was discovered using the cathode ray?
How did Thomson describe the atom?
What did Rutherford do and how did it change the atomic theory?
Give the 3 sub-atomic particles their charge and location.
What does atomic number represent?
What is the mass number?
Describe isotopes.
What is a mole?
Define molar mass.
How many moles of oxygen atoms are in 64 g of oxygen?
Calculate the number of g contained in 14 moles of helium.
How many atoms are in 3 moles of gold?
How are wavelength and frequency related?
What’s the energy of a photon of light?
Give Bohr’s model of an atom.
Is Bohr’s model useful for all atoms?
How do electrons travel?
How is Quantum theory different from Bohr?
Give the quantum numbers.
Sketch a s orbital and a p orbital.
What is the electron configuration for Al? S?
Give the Aufbau principle, Hund’s rule, and Pauli exclusion principle.
Describe the valence electrons versus the core electrons.
How is the noble gas notation different than the regular electron configuration?
Use the noble gas method for Sn and Ba.
How many shapes are there if n = 3? How many totals orbitals?
How many possible electrons if n = 4?
Chp 5,6 Review
What did Mendleev do?
How did Moseley change Mendleev’s idea?
What set of elements were totally left off of Mendleev’s table?
Where are the Lanthanides and Actinides?
Sketch the periodic table and label the different blocks.
Give the names for the following families
#1
#2
#17
#18
What is the name for the d block elements?
Define the following properties and give their periodic trends
Atomic Radii
Ionization Energy
Electron Affinity
Ionic Radii
Electronegativity
How are covalent bonds formed? Ionic?
Explain the difference between polar and nonpolar covalent bonds.
What is a molecular formula?
Give an example of a diatomic molecule.
State the Octet rule.
What are lone pair electrons?
Draw lewis dot structures for the following
H2S
SO3
H2SO4
CO2
What is meant by resonance? Can it always happen?
Why is NaCl not the true representation for sodium chloride as a solid?
What are polyatomic ions?
Explain the “sea of electrons” idea for metals.
What 2 things are required for molecules to be polar?
What is the VSEPR theory?
Give the names of the shapes of molecules below
HI
BF3
CI4
NH3
H2O
SO2
What is hybridization?
How many sets of electrons are around the central atom if its sp3 hybridized? Sp2?
Give the 3 intermolecular forces and their relative strength.
Why is water a liquid even though it is very small for a molecule?
Chp 6, 7 Rev.
1)
What are the two types of chemical bonds?
2)
Describe Polar and Non-polar bonds.
3)
What is the octet rule?
4)
Draw lewis dot structures for the following chemicals;
a) H20
b) CH4
c) SO2
d) SO4 2-
5)
Define resonance.
6)
How are ionic compounds different from molecular compounds?
7)
8)
How do metals bond?
What are the shapes for the following;
a) H20
b) CH4
c) SO2
d) SO4 2-
9)
State the VSEPR theory.
10)
List the intermolecular forces by increasing strength.
11)
Name the following compounds
a) LiCl
b) NaOH
c) FeI3
d) CuNO3
e) C2S3
f) SO2
g) HF
h) HFO3
i) H2SO3
12)
What is the formula mass for H2O? It’s molar mass?
13)
How many grams are in 5 moles of water?
14)
What is the percent composition of water?
15)
Calculate the empirical formula for 78g of B and 22g of H.
16)
What do you need to know to calculate the molecular formula for #15?
Chp 22 Rev
1) Describe the five types of radioactive decay.
2) What is meant by half-life?
3) If a sample starts at 200g how much will be left after 5 half-life’s have gone by?
4) Why doesn’t an atom’s mass equal the masses of all the particles added together
in it’s structure?
5) Write a reaction for Carbon -12 giving off an alpha particle.
6) Write a reaction for Carbon – 12 giving off a beta particle.
7) Write a reaction for Carbon – 13 absorbing an electron.
8) What is created when an atom goes through fission?
9) How can radioactive decay be used to date a sample of bone found in an
archeological dig site?
10) Define
a. Critical mass
b. and Chain reaction.