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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. If G is negative - is the reaction spontaneous?
Lemon yellow
Periods 8 and 9 - lanthanides and actinides
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Yes

2. Gibb's Free Energy equation
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
DG = DH - TDS
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

3. Isotope
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
The solute is dissolved in the solvent.
Same element - different number of neutrons
More active element replaces less active element in a compound.

4. Dalton's Law
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Pressure of mixture of gases equals some of individual gas pressures.
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
OH - alcohols - name ends in ol

5. Gamma decay
Classified as strong bases but not very soluble.
2 bonding - 1 nonbonding
Liquid at room temperature - used to make gasoline and solvents
Emission of electromagnetic energy after beta - positron - or alpha decay

6. Positron emission
Disordered systems with higher entropies are favored
Yellow
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

7. pewter
Spin is +1/2 or -1/2 in an orbital
Degrade the oxone layer
21% of atmosphere - colorless - odorless - supports combustion reactions
Mixture of tin - copper - bismuth - and antimony

8. Beta particle
No
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Mixture of copper - zinc - and other metals
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

9. Sulfate ion
SO4²?
Largest radioactive particle - decrease atomic number by 2 and the atomic mass by 4 - range of 5 cm in air - high energy and velocity - 100 -000 ionizations per cm
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

10. Hydroxyl group
4.5 to 8.3 - Red to blue
M1V1 = M2V2
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
OH - alcohols - name ends in ol

11. What kind of bonds generally hold gases together?
3.1 - 4.4 - red to yellow
Covalent
Make up jet fuels and kerosene
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

12. Coal
Q = mcDT
Degrade the oxone layer
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Mixture of silver and copper

13. Ionization energy
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Lemon yellow
1st group - most reactive metal family - react violently with water - create basic solutions
Orange

14. Ethers
R-O-R functional group - shorter chain ends in oxy - other is ane
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Oxide that reacts with water to form either an acid or a base
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

15. Formula for calculating enthalpy change with bond energies
V1/T1 = V2/T2
DH = bonds broken - bonds formed
Potassium - Calcium - Sodium
Same molecule - different electron pair positions

16. Is removing an electron an exothermic or endothermic process?
Endothermic
Purple/pink
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
4 bonding - 109.5° - sp³ hybridization

17. What 3 metals will react with cold water?
Acid to water
Potassium - Calcium - Sodium
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
The solute is dissolved in the solvent.

18. Fusion
No
P1/V1 = P2/V2
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

19. Halogen properties
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Purple/pink
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Increase right and up

20. Properties of acids
3 bonding - 1 nonbonding 107°
White
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
Magnesium

21. Metallic bonds
Electrons are free to move through metal structure - high conductivity - ductile
Magnesium
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Blue-green

22. Complete combustion occurs when there is
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Excess oxygen
No
C2H3O2?

23. bronze
6 bonding - 90° - sp³d2² hybridization
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Mixture of copper - zinc - and other metals
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

24. Sulfide color: CuS - HgS - and PbS
Deadly - yellow-green - weapon
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Black
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

25. What kind of bonds generally hold liquids together?
Covalent
White
Glass and plastic
Soluble

26. Isomer
Insoluble
Lemon yellow
Same formula - different structure
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

27. Carbonate ion
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
CO3²?
Yes in thermo - no in electro
Yellow

28. Electron affinity
Potassium - Calcium - Sodium
Low pressures - high temperatures
No
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

29. Add acid to water or water to acid
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Acid to water
More active element replaces less active element in a compound.
COH functional group - name ends in -al

30. Properties of molecular crystals and liquids

31. Hydrofluoric acid is used for
NO3?
Decreased
Orientation of orbital in space
Etching glass and frosting lightblubs

32. Carbon dioxide gas properties
Miscible with water - flammable - used as fuel - poisonous
Soluble
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

33. Exceptions to the octet rule
Yes
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
DH = bonds broken - bonds formed
Miscible with water - flammable - used as fuel - poisonous

34. Compounds with 12-18 carbons
CO - produced from incomplete combustion - very toxic
Two compound react to form two new compounds
Make up jet fuels and kerosene
2nd group - fairly reactive - pastes are used in batteries

35. Color of excited Li+ - Sr2+ - Ca2+
6 bonding - 90° - sp³d2² hybridization
Red
3 bonding - 1 nonbonding 107°
Two compound react to form two new compounds

36. Compounds with 1-4 carbons
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Energy level - as it increases electrons are less bound to the nucleus
Gases at room temperature - used for fuel
SO4²?

37. Color of CrO7²? solution
Orientation of orbital in space
COH functional group - name ends in -al
Orange
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

38. Sulfide color: As2S3
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
2 bonding - 180° - sp hybridization
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Lemon yellow

39. Sigma bonds
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
CO - produced from incomplete combustion - very toxic
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Disordered systems with higher entropies are favored

40. Sulfide color: ZnS
Moles of solute / kg solvent
Two reactants combine to form a single product
Nonmetal oxides form acids - metal oxides form bases
White

41. Molarity
R-O-R functional group - shorter chain ends in oxy - other is ane
Properties of solutions that depend on the number of particles per solvent molecule
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Moles / L

42. How can hydrogen be produced?
Purple
Same element - different number of neutrons
Orange
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

43. Steel
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Mixture of iron and carbon
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Blue-green

44. Nitrate ion
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
NO3?
Oxide that reacts with water to form either an acid or a base
The solute is dissolved in the solvent.

45. F compounds are...
ClO3?
Soluble
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
Soluble except when containing alkaline earth metals

46. Metallic solids
NH2 - ends in -amide
Diamond - graphite - amorphous - fullerenes
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
CO - produced from incomplete combustion - very toxic

47. Bent
2 bonding - 1 nonbonding
SO4²?
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
M1V1 = M2V2

48. Bromthymol blue: pH range and colors
Gas pressure = atm pressure - height of mercury
8.3 to 10.0 - colorless to pink
DH = bonds broken - bonds formed
6.0 to 7.6 - yellow to blue

49. Noble gases
Make up jet fuels and kerosene
Mixture of silver and copper
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Extremely slow reactivity

50. Suspension
Orange
Mixture of copper and zinc
Deadly - yellow-green - weapon
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent