1. CHEMISTRY SOL REVIEW
DAY 1

2. UNIT 2 - Matter Matter is anything with mass & _______ Volume
____ substances are types of matter with definite & uniform characteristics.
Pure
For example, _____ contain only one kind of atom.
Elements

3. UNIT 2 - Matter
A _____ is another pure substance that is made of more than one type of atom & can only be broken down by chemical means.
Compound
_______ are types of matter with 2 or more substances that can vary in composition & properties
Mixtures

4. UNIT 2 - Matter
A _______ mixture has a uniform composition (Stainless steel, KoolAid)
Homogeneous
_____ is considered the universal solvent
Water
The particles dissolved in a solvent are called the __________
Solutes
A _____ is really a heterogenous mixture but LOOKS like a solution (milk)

5. UNIT 2 - Matter Phase changes are _____ changes (physical or chemical)
The process of a solid becoming a gas (without becoming a liquid first) is ___
Sublimation
What state of matter has the strongest IMF?
Solid

6. UNIT 2 - Matter
Name the 4 things used as evidence of a chemical reaction occurring
Production of a gas (odor or bubbles)
Color change
Release/absorption of energy (light or heat)
Forming a precipitate (chunks )
Name a way to separate a mixture
Filtration, distillation, chromatography, centrifuging, decanting

7. UNIT 3 – History of the Atom
5 part atomic theory – all matter made of atoms
Dalton
Cathode Ray Tube experiments, Plum Pudding model, Electrons have mass & a negative charge
JJ Thomson

8. UNIT 3 – History of the Atom
Passed alpha particles through gold foil and found that the nucleus is dense and positively charged
Rutherford
Electrons found in levels or shells around the nucleus
Bohr
An electron passed through an electric field will bend ____
Toward the positive

9. UNIT 3 – History of the Atom
Atomic number gives us # of ____ in an atom of each element
Protons
Mass number is calculated by adding __
Protons plus neutrons
Different isotopes have different #s of __
Neutrons
Different __ have different #s of electrons
Ions

10. UNIT 3 – History of the Atom
Calculate the average atomic mass of copper if copper has 2 isotopes % has a mass of amu and the rest has a mass of amu.
(.691 * 62.93) + (.309 * 64.93)
63.55
Flourine – 19 has how many neutrons? 10
What is the molar mass of carbon?

11. UNIT 3 – History of the Atom
You find an artifact with a C-14:C-12 ratio that is 1/16 the modern ratio. The half life of C-14 is 5715 years. How old is the artifact?
22860 years
Alpha, Beta, & Gamma particles are all given off by radioactive decay. Why are gamma rays the most dangerous? (Answer should involve size & penetration)
Tiny so they can penetrate the farthest – only stopped by lead

12. UNIT 4 – Electron Configuration
What is the longhand electron configuration for N?
1s2 2s2 2p3
For Fe?
1s2 2s2 2p6 3s2 3p6 4s2 3d6
What is the shorthand config for Ca?
[Ar] 4s2
The electrons in the outermost shell are called the _______ electrons
Valence

13. UNIT 4 – Electron Configuration
How many p orbitals are there? 3
What shape is a p orbital?
Bowtie or dumbbell or figure 8
How many electrons can be held in d orbitals? 10

14. UNIT 4 – Electron Configuration
How many valence electrons does oxygen have? 6
The rows in the periodic table are called
Periods
Draw a Lewis dot diagram for Nitrogen
When an electron returns to its ground state after being excited, it releases energy and emits a _____, or a particle of light.

15. Unit 5 – The Periodic Table
The elements on the right side of the staircase are _____
Nonmetals
The first column or group of elements are called the ____
Alkali metals
Group 7 is called the ___
Halogens

16. UNIT 5 – The Periodic Table
The d-group elements are called the __
Transitional metals
The f-block elements are called the ___
Inner transition metals
What happens to atomic radius as you move from top to bottom down the periodic table?
Gets bigger

17. UNIT 5 – The Periodic Table
The energy required to remove an electron from an atom is called __
Ionization energy
What happens to ionization energy as you move from left to right across a period?
Gets bigger
An atoms affinity for electrons in a compound is called its ___
Electronegativity

18. ANNOYING 2009 Question
Potassium (K) has a smaller atomic mass than (Ar) even though the atomic number of potassium is larger than the atomic number of argon. Which of the following BEST accounts for this observation?
F At STP, K is in the solid phase, but argon is gas
G It is easier for a potassium atom to lose an electron than it is for an argon atom
H The most common isotopes of argon have more protons than the most common isotopes of potassium.
J The most common isotopes of potassium have fewer neutrons than the most common isotopes of Ar J