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SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. How can hydrogen be produced?
yellow
Disordered systems with higher entropies are favored
Most stable
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

2. Examples of amorphous solids
Glass and plastic
Solid at room temperature
Potassium - Calcium - Sodium
Black

3. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
NO3?
Soluble
PV = nRT - R = .0821

4. Phosphate ion
Periods 8 and 9 - lanthanides and actinides
PO4³?
P1/V1 = P2/V2
Stronger

5. Halogen properties
R-O-R functional group - shorter chain ends in oxy - other is ane
Solid at room temperature
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

6. Properties of acids
Same molecule - different electron pair positions
Increases left and down
1. Water solutions conduct electricity 2. Will react with metals more active than hydrogen to liberate hydrogen. 3. Change litmus to red 4. Phenolphthalein is colorless 5. React with bases to form water and salt 6. React with carbonates to release ca
Make up jet fuels and kerosene

7. London dispersion forces
NH2 - ends in -amide
Strong acids - strong bases - soluble salts
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
More active element replaces less active element in a compound.

8. Spin quantum number (ms)
ClO3?
Spin is +1/2 or -1/2 in an orbital
Emission of electromagnetic energy after beta - positron - or alpha decay
Solution where particles are between 100 and 1000 nm in size—particles this small will not settle.the particles cannot be filtered - but they do scatter light

9. What is the equation used for heat transfer problems?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
More active element replaces less active element in a compound.
Q = mcDT
Electrons are free to move through metal structure - high conductivity - ductile

10. Sulfide color: CdS
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Bright yellow
OH - alcohols - name ends in ol

11. Carbonate ion
CO3²?
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Make up jet fuels and kerosene
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

12. Dalton's Law
Pressure of mixture of gases equals some of individual gas pressures.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Gas pressure = atm pressure + height of mercury
Blue-green

13. Gibb's Free Energy equation
DG = DH - TDS
Oxide that reacts with water to form either an acid or a base
Moles of solute / kg solvent
Moles / L

14. Alkali Metals
NH2 functional group - name ends in -amide
1st group - most reactive metal family - react violently with water - create basic solutions
3 bonding - 120° - sp² hybridization
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

15. Sulfate ion
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Photography
SO4²?
Decreased

16. Compounds with 1-4 carbons
No two electrons can have the same set of 4 quantum numbers
4.184
Gases at room temperature - used for fuel
NO3?

17. Allotropic forms of carbon
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Degrade the oxone layer
Diamond - graphite - amorphous - fullerenes
OH - alcohols - name ends in ol

18. Chlorate ion
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Blue-green
Periods 8 and 9 - lanthanides and actinides
ClO3?

19. Alkaline earth metals
Solution where particles are between 100 and 1000 nm in size—particles this small will not settle.the particles cannot be filtered - but they do scatter light
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
2nd group - fairly reactive - pastes are used in batteries
Most stable

20. Methanol
Lemon yellow
Miscible with water - flammable - used as fuel - poisonous
A compound breaks into two parts
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

21. Steel
Substance can act either as an acid or a base
Mixture of iron and carbon
Soluble
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

22. Color of excited Cu2+
Involves water
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Blue-green

23. General properties of alloys
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Solution where particles are between 100 and 1000 nm in size—particles this small will not settle.the particles cannot be filtered - but they do scatter light
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
OH - alcohols - name ends in ol

24. Incomplete combustion occurs when there is
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Increases left and down
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Limited oxygen

25. Boyle's Law
4.5 to 8.3 - Red to blue
Do not conduct electricity well
P1/V1 = P2/V2
Same molecule - different electron pair positions

26. Color of CrO7²? solution
Orange
Low pressures - high temperatures
8.3 to 10.0 - colorless to pink
Etching glass and frosting lightblubs

27. Is removing an electron an exothermic or endothermic process?
Mixture of iron and carbon
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Endothermic
COOH - ends in -oic acid

28. Anhydride
Oxide that reacts with water to form either an acid or a base
4.184
Heat required to make a substance melt.
yellow

29. Chlorine gas
Two compound react to form two new compounds
Deadly - yellow-green - weapon
COOH - ends in -oic acid
Involves water

30. Carbon dioxide gas properties
NO3?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Increased

31. Litmus: pH range and colors
Deadly - yellow-green - weapon
4.5 to 8.3 - Red to blue
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Mixture of silver and copper

32. Solute vs. Solvent
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
C2H3O2?
21% of atmosphere - colorless - odorless - supports combustion reactions
The solute is dissolved in the solvent.

33. Alkali metal properties
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
DG = DH - TDS
Gold

34. Decomposition reaction
A compound breaks into two parts
Covalent
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
COOH - ends in -oic acid

35. Carboxylic acid
Purple/pink
COOH functional group - name ends in oic acid
Q = mcDT
Light green

36. Combustion reaction
Stronger
Yes in thermo - no in electro
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
DG = DH - TDS

37. What is the ideal gas law?
1st group - most reactive metal family - react violently with water - create basic solutions
PV = nRT - R = .0821
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Soluble except when containing Ag? - Hg2²? - or Pb²?

38. Octahedral
Endothermic
6 bonding - 90° - sp³d2² hybridization
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
More active element replaces less active element in a compound.

39. Molarity
Moles / L
COOH functional group - name ends in oic acid
Decreased
Mixture of copper - zinc - and other metals

40. Magnetic quantum number (ml)
Orientation of orbital in space
Solution where particles are between 100 and 1000 nm in size—particles this small will not settle.the particles cannot be filtered - but they do scatter light
1. Solids don't conduct good electrical current. 2. Liquid phase are good conductors 3. Relatively high melting and boiling points 4. Do not vaporize readily at room temperature. 5. Brittle / easily broken 6. Soluble in water
Etching glass and frosting lightblubs

41. amphoteric
Non-polar if electronegativity difference is between 0 and 0.4 - in polar bonds the atom with more electronegativity has greater pull on electrons. Single bond is a sigma bond - double and triple bonds have one sigma - and the other are pi bonds.
CO - produced from incomplete combustion - very toxic
PO4³?
Substance can act either as an acid or a base

42. What are the factors that affect reaction rate?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Same molecule - different electron pair positions
Stronger

43. Principal quantum number (n)
Gold
Mixture of tin - copper - bismuth - and antimony
2 bonding - 1 nonbonding
Energy level - as it increases electrons are less bound to the nucleus

44. Positron emission
Do not conduct electricity well
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
1st group - most reactive metal family - react violently with water - create basic solutions
Light green

45. Boiling point elevation formula
Electrons are free to move through metal structure - high conductivity - ductile
4 bonding - 109.5° - sp³ hybridization
Periods 8 and 9 - lanthanides and actinides
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

46. Color of excited Na+
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Moles / L
yellow
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

47. Amine
NH2 functional group - name ends in -amide
Gold
DG = DH - TDS
Electrons are free to move through metal structure - high conductivity - ductile

48. Name the six strong acids
Two atoms with the same number of electrons
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
No two electrons can have the same set of 4 quantum numbers
Blue

49. Fusion
Non-polar if electronegativity difference is between 0 and 0.4 - in polar bonds the atom with more electronegativity has greater pull on electrons. Single bond is a sigma bond - double and triple bonds have one sigma - and the other are pi bonds.
Gold
Properties of solutions that depend on the number of particles per solvent molecule
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

50. Exceptions to the octet rule
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
COOH functional group - name ends in oic acid
Solution where particles are between 100 and 1000 nm in size—particles this small will not settle.the particles cannot be filtered - but they do scatter light
Periods 8 and 9 - lanthanides and actinides