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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. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
ClO3?
Insoluble
Photography
7th group - form salts - always exist as diatomic molecules - used in modern lighting

2. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Stronger
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Properties of solutions that depend on the number of particles per solvent molecule

3. Ionization energy
CO - produced from incomplete combustion - very toxic
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
3 bonding - 120° - sp² hybridization
Lemon yellow

4. Color of CrO7²? solution
Orange
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Make up jet fuels and kerosene
Electrons are free to move through metal structure - high conductivity - ductile

5. Ionic bond
1. don't conduct good current 2. many exist as gases at room temp 3. melting points of solid crystals are low 4. large amount of energy needed to decompose
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
yellow

6. Properties of molecular crystals and liquids

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7. Equation when using a barometer to calculate gas pressure.
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Gas pressure = atm pressure - height of mercury
Gas pressure = atm pressure + height of mercury
2 bonding - 1 nonbonding

8. Nitrate ion
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Two atoms with the same number of electrons
NO3?
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

9. Ammonium Ion
More active element replaces less active element in a compound.
Moles / L
NH4?
COOH - ends in -oic acid

10. Trigonal planar
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
Nonmetal oxides form acids - metal oxides form bases
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
3 bonding - 120° - sp² hybridization

11. Acids with more oxygen atoms are
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
4 bonding - 109.5° - sp³ hybridization
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Stronger

12. Synthesis reaction
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Two reactants combine to form a single product
Blue
Light green

13. General Properties of Organic Compounds
Solid at room temperature
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

14. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
1. don't conduct good current 2. many exist as gases at room temp 3. melting points of solid crystals are low 4. large amount of energy needed to decompose
6 bonding - 90° - sp³d2² hybridization

15. Name the six strong acids
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

16. Color of excited Li+ - Sr2+ - Ca2+
Mixture of iron and carbon
ClO3?
Red
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

17. Alchohols
OH functional group - name ends in -ol
Disordered systems with higher entropies are favored
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
COOH functional group - name ends in oic acid

18. What is the ideal gas law?
yellow
It is at equilibrium
3 bonding - 120° - sp² hybridization
PV = nRT - R = .0821

19. Radioactivity
Do not conduct electricity well
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Extremely slow reactivity
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

20. Fusion
4 bonding - 109.5° - sp³ hybridization
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
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

21. Anhydride
CO3²?
CO - produced from incomplete combustion - very toxic
Oxide that reacts with water to form either an acid or a base
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

22. What kind of bonds generally hold liquids together?
It is at equilibrium
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Covalent
More active element replaces less active element in a compound.

23. Alkali metal properties
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
More active element replaces less active element in a compound.
Orange

24. Colligative properties
Soluble except when containing alkaline earth metals
Light green
Mixture of copper - zinc - and other metals
Properties of solutions that depend on the number of particles per solvent molecule

25. Exceptions to the octet rule
Mixture of silver and copper
C2H3O2?
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Gas pressure = atm pressure - height of mercury

26. Covalent-network / atomic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
6 bonding - 90° - sp³d2² hybridization
NH4?
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.

27. Supersaturated solution
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
SO4²?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

28. Complete combustion occurs when there is
Two compound react to form two new compounds
PO4³?
Photography
Excess oxygen

29. bronze
Bright yellow
Mixture of copper - zinc - and other metals
Deadly - yellow-green - weapon
7th group - form salts - always exist as diatomic molecules - used in modern lighting

30. If G is positive - is the reaction spontaneous?
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
No
Miscible with water - flammable - used as fuel - poisonous

31. Fission
Classified as strong bases but not very soluble.
Soluble
5 bonding - 90° and 120° - sp³d hybridization
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

32. Suspension
More active element replaces less active element in a compound.
Acid to water
C2H3O2?
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

33. Hydroxyl group
DG = DH - TDS
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
OH - alcohols - name ends in ol
COOH functional group - name ends in oic acid

34. Ethanol
Bright yellow
NH4?
Two compound react to form two new compounds
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

35. Bromthymol blue: pH range and colors
OH functional group - name ends in -ol
Mixture of copper and zinc
6.0 to 7.6 - yellow to blue
4.184

36. Compounds with 5-10 carbons
Energy level - as it increases electrons are less bound to the nucleus
White
Emission of electromagnetic energy after beta - positron - or alpha decay
Liquid at room temperature - used to make gasoline and solvents

37. Litmus: pH range and colors
Increased
ClO3?
4.5 to 8.3 - Red to blue
CO - produced from incomplete combustion - very toxic

38. Decomposition reaction
ClO3?
A compound breaks into two parts
Mixture of tin - copper - bismuth - and antimony
Insoluble

39. Isoelectronic
Two atoms with the same number of electrons
Spin is +1/2 or -1/2 in an orbital
4.5 to 8.3 - Red to blue
Orange

40. Define heat of fusion.
Heat required to make a substance melt.
Increase right and up
NH2 - ends in -amide
Mixture of silver and copper

41. Carbonate ion
Gas pressure = atm pressure - height of mercury
Light green
Orange
CO3²?

42. Graham's Law
CO3²?
Gold
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Lemon yellow

43. Molality
Moles of solute / kg solvent
Increase right and up
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
ClO3?

44. Methyl orange: pH range and colors
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
Gold
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
3.1 - 4.4 - red to yellow

45. Carbon monoxide
Disordered systems with higher entropies are favored
Soluble
CO - produced from incomplete combustion - very toxic
Nonmetal oxides form acids - metal oxides form bases

46. Isotope
Same element - different number of neutrons
OH functional group - name ends in -ol
PO4³?
Spin is +1/2 or -1/2 in an orbital

47. Acetate ion
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Heat required to make a substance melt.
C2H3O2?
7th group - form salts - always exist as diatomic molecules - used in modern lighting

48. F compounds are...
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Orange
Soluble except when containing alkaline earth metals
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

49. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Covalent
Mixture of silver and copper
Soluble

50. Phosphate ion
PO4³?
Glass and plastic
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
NH2 functional group - name ends in -amide