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Chemistry MSL Review
Random Stuff:
What is the difference between a chemical change and a physical change?
Distinguish between accuracy and precision.
Atomic Structure
Isotopes and Average Atomic Mass
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They are from another worksheet. Write the location on of each of the following families or classifications of elements on a periodic table: metals, nonmetals, ...
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Chemistry MSL Review Random Stuff: What is the difference between a chemical change and a physical change? Distinguish between accuracy and precision.
Atomic Structure
Isotopes and Average Atomic Mass
Nomenclature Review:
The Periodic Table:
The letters inside the table have no significance here. They are from another worksheet.
Write the location on of each of the following families or classifications of elements on a periodic table: metals, nonmetals, metalloids, alkali metals, alkaline earth metals, halogens, noble gases, transition metals, & diatomic elements.
- Horizontal rows are called ______________
- Columns are called ___________ or ____________
- Name group 1___________, 2 ________________, 3-12______________, 17__________________, 18________________.
- Elements are arranged according to their __________________
- Elements within a group have the same number of ____________________
- Name the groups with the following ionic charges: +1____, +2____, +3____, -3____, -2____, -1____.
- Label Zn and Ag with their charges.
- As you go across the periodic table, the elements go from ( metals / nonmetals ) to ( metal / nonmetals ).
- Draw in the metalloid line. Mark the six metalloids (semimetals).
- Where are the s, p, d and f sublevels?
- Where are the most active metals?
Lewis dot diagrams
- Calcium 5. e 2. Potassium 6. Carbon 3. Argon 7. oxygen 4. Aluminum 8. Helium
Atomic Theory A. Dalton’s Theory
- All matter is composed of ________.
- Atoms of the same element are the same and are _________ from atoms of other elements.
- Atoms cannot be subdivided, _______, nor _________.
- Atoms combine in whole number ________.
- Atoms in chemical reactions are combined, separated, or _________.
B. Thompson and Millikan had negative attitudes. Thompson discovered the ______________ and Millikan said it had very little __________. C. Rutherford said the nucleus is ____________ and _________________.
D. Bohr proposed the photon emission model which explained the characteristic line emission spectrum.
E. When an electron goes from n=2 to n=1 what happens? ________...... Electromagnetic Spectrum: Use the electromagnetic spectrum to relate wavelength and energy. c = λν E = hν What is the energy of a photon with a wavelength of 9.0 x 10^9 nm? Explain what is meant by the wave‐particle nature of light. Are the colors of flame tests due to taking in energy or releasing energy? Explain What does it mean when we say energy levels are quantized?
What are the essential points of Bohr’s theory of the structure of the hydrogen atom?
Chemical bonding Classify the following as ionic (metal/cation + nonmetal/anion), covalent (nonmetal and nonmetal).
- CaCl 2 5. NH 4 Cl
- CO 2 6. KI
- BaSO 4 7. NO 2
- K 2 O 8. NaOH
Shapes of molecules The VSEPR theory helps us predict the shape of molecules. The unshared pairs of electrons will push the shared pairs away and change the shape of the molecule. Determine the shapes of the following by first drawing the lewis dot structures for them and drawing the dipole moments on each polar covalent bond. This will allow you to determine the shape and molecular polarity: N 2 , H 2 O, CO 2 , NH 3 , CH 4 , SO 3 , H 2 S, CH 3 Cl {Linear, Bent, Trigonal Planar, Pyramidal, Tetrahedral
Polarity In polar covalent bonds the electrons are not shared equally. When the electronegativity difference is great enough (above 0.3) and the shape is asymmetrical, the molecule will be polar.
Determine if the examples from above are polar or nonpolar.
Metallic Bonding: Describe the properties of metals and how their mobile electrons contribute to these properties. What is an alloy (Explain and given an example)?
The MOLE
- Determine the number of moles of 25 g of NaCl.
- Determine the number of grams of 2.5 mol NaCl.
- What volume will 3.2 moles of Os occupy at STP?
- How many moles of hydrogen are needed to completely react with two moles of nitrogen?
5. The average kinetic energy of gas particles depends on temperature.
A. Which of the above are not completely true but accepted anyway?
An ideal gas will behave like a real gas when the TEMPERATURE IS LOW (slow moving particles are attracted to each other – hey baby) and the PRESSURE IS HIGH (particles can get close enough to bond - let’s become a liquid. ).
Gases expand to fill their containers, they are fluid, have low density, are compressible, diffuse and effuse.
Density D = mass Volume
Gas Laws
Phase Diagram
- What section represents the solid phase? Liquid? Gas?
- Describe what line d-f represents.
- Describe what line d-e represents.
- Describe what line d-g represents.
- What is the substance’s normal melting point? Boiling Point?
- When do all three phases exist at once?
- Would an increase in pressure cause this substance to freeze or melt?
Heating and Cooling Curves
Change the temperatures to make these curves be for water.
- What is a? b? c? d? e?
- When does KE change?
- When does PE change?
- Which direction in endothermic? Exothermic?
- Would the ∆T for an endothermic reaction be positive or negative?
- What equation would solve for heat during lines a, c, e?
- What equation would solve for heat during d? b?
- What does it mean that the specific heat of water is more than the specific heat of ice?
- What is the difference between temperature and heat?
Electrolytes Solutes with charges will conduct electricity and are therefore electrolytes. Electrolytes include:
- Ionic solutes:
- Strong Acids:
- Strong Bases:
Molarity
M = moles of solute Liters of solution
- What is the molarity of a solution in which 10 g of silver nitrate (AgNO 3 ) is dissolved in 500 mL of solution?
Acids and Bases What are the three different definitions of acids and bases? Acids: H+ / proton donors (electron pair acceptors) Bases: H+ / proton acceptors (electron pair donors)
Explain the significance of these diagrams in relation to pH.
Determine the pH, pOH, [H 3 O+], and [OH-] for each of the following given.
1. [H 3 O+]= 0.500 M.
2. pOH = 3.
3. [OH-] = 1.50 x 10-5^ M.
4. pH = 2.
5. [OH-] = 3.2 x 10-8^ M.
Calculate the molarity of an acetic acid solution if 34.57 mL of this solution are needed to neutralize 25.19 mL
of 0.1025 M sodium hydroxide.
Reaction Rate
The speed of the reaction OR The change in concentration of reactants over time.
Factors affecting rate;
- Type of reactants
- Surface area
- Temperature
- Concentration of reactants
- Catalysts: a substance that lowers the activation energy of a chemical reaction. ∆E = ∆H = ENTHALPY = heat of the reaction = Eproducts - Ereactants
Exothermic ∆H = is negative Endothermic ∆H = is positive
- Are the forward reactions endothermic or exothermic?
- Which has more energy, reactants or products?
- What does the catalyst do?
- Is the catalyst part of the rxn?
- Is ∆H for this forward rxn positive or negative? How do you know? ENTROPY = ISDORDRE (Get it?) DISORDERLY = Gases > Solutions > Liquids > Solids = ORDERLY DISORDERLY = 2 compounds > 1 compound = ORDERLY
Facts about Reactions Indications that a reaction has taken place are 1. 2. 3. 4. Nuclear Decay Describe the characteristics symbols masses Shielding / penetrating ability Alpha
Beta Gamma
Predict the products of the nuclear reactions
Concept of half-life:
Silicon‐31 has a half‐life of approximately 2.5 hours. If we begin with a sample containing 2000 kg of Si‐31, what is the approximate amount remaining after 10 hours?
Carbon‐15 has a half‐life of 5.0 seconds. Suppose we have a sample containing 100 grams of Carbon‐15. How much will remain after 30 seconds?
Define Fission
Define Fusion
How does a nuclear reactor work?