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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.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. Gibb's Free Energy equation
Involves water
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Two atoms with the same number of electrons
DG = DH - TDS

2. Alpha particle
Make up jet fuels and kerosene
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
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
White

3. Spin quantum number (ms)
Disordered systems with higher entropies are favored
2 bonding - 180° - sp hybridization
Black
Spin is +1/2 or -1/2 in an orbital

4. Ionic bond
PO4³?
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Solid at room temperature
Gas pressure = atm pressure - height of mercury

5. Ammonium Ion
Insoluble
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
NH4?

6. Fission
3 bonding - 120° - sp² hybridization
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.
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

7. Dilution equation
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
M1V1 = M2V2
Increases left and down
More active element replaces less active element in a compound.

8. Coal
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
4.184
Most stable
2 bonding - 1 nonbonding

9. What metal will react in hot water?
Magnesium
Solid at room temperature
Lemon yellow
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

10. Incomplete combustion occurs when there is
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
Limited oxygen
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

11. Single Replacement / displacement reaction
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
More active element replaces less active element in a compound.
COH functional group - name ends in -al
Mixture of silver and copper

12. What is the equation used for heat transfer problems?
Yes in thermo - no in electro
Electrons are free to move through metal structure - high conductivity - ductile
Q = mcDT
White

13. Sulfide color: ZnS
Etching glass and frosting lightblubs
White
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Low pressures - high temperatures

14. Isoelectronic
Substance can act either as an acid or a base
Light green
Two atoms with the same number of electrons
Increase right and up

15. If G is positive - is the reaction spontaneous?
No
Do not conduct electricity well
Same formula - different structure
Yes

16. Gamma decay
White
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Properties of solutions that depend on the number of particles per solvent molecule
Emission of electromagnetic energy after beta - positron - or alpha decay

17. What is the second law of thermodynamics?
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Increased
NH4?
Disordered systems with higher entropies are favored

18. Covalent-network / atomic solids
Oxide that reacts with water to form either an acid or a base
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Covalent
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

19. When a reaction is endothermic - the entropy is
2 bonding - 180° - sp hybridization
Black
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Increased

20. Phenolphthalein: pH range and colors
Soluble except when containing Ag? - Hg2²? - or Pb²?
8.3 to 10.0 - colorless to pink
3 bonding - 1 nonbonding 107°
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

21. Color of excited Na+
Mixture of tin - copper - bismuth - and antimony
21% of atmosphere - colorless - odorless - supports combustion reactions
Green
yellow

22. Color of Fe3+ solution
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
NH2 functional group - name ends in -amide
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Yellow to orange

23. Hydrogen gas properties
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
3.1 - 4.4 - red to yellow
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
OH functional group - name ends in -ol

24. When are gases MOST ideal?
Yellow
Low pressures - high temperatures
C2H3O2?
Soluble except when containing alkaline earth metals

25. Magnetic quantum number (ml)
Orientation of orbital in space
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
2 bonding - 1 nonbonding
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.

26. Carboxylic acid group
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.
Same formula - different structure
Red
COOH - ends in -oic acid

27. Color of Ni2+ solution
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Green
Soluble except when containing alkaline earth metals
Red

28. Color of Cu2+ solution
CO - produced from incomplete combustion - very toxic
Blue
Limited oxygen
Increased

29. Decomposition reaction
Mixture of copper - zinc - and other metals
A compound breaks into two parts
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
OH functional group - name ends in -ol

30. Positron emission
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
2 bonding - 180° - sp hybridization
Q = mcDT
COOH - ends in -oic acid

31. What kind of bonds generally hold gases together?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
OH functional group - name ends in -ol
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Covalent

32. Sulfide color: As2S3
It is at equilibrium
Lemon yellow
Classified as strong bases but not very soluble.
5 bonding - 90° and 120° - sp³d hybridization

33. If G is negative - is the reaction spontaneous?
Magnesium
DH = bonds broken - bonds formed
Light green
Yes

34. Linear
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Light green
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 bonding - 180° - sp hybridization

35. Complete combustion occurs when there is
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Excess oxygen
Gas pressure = atm pressure - height of mercury
ClO3?

36. Ketone
6.0 to 7.6 - yellow to blue
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

37. Charles' Law
Potassium - Calcium - Sodium
V1/T1 = V2/T2
Heat required to make a substance melt.
Soluble

38. Color of excited Ba2+
NH2 functional group - name ends in -amide
Photography
Strong acids - strong bases - soluble salts
Light green

39. Colligative properties
Purple
Properties of solutions that depend on the number of particles per solvent molecule
Liquid at room temperature - used to make gasoline and solvents
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

40. Acetate ion
Substance can act either as an acid or a base
More active element replaces less active element in a compound.
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
C2H3O2?

41. When the reaction is exothermic - the entropy is
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Same element - different number of neutrons
Decreased
PO4³?

42. Color of excited Cu2+
Substance can act either as an acid or a base
Heat required to make a substance melt.
Mixture of iron and carbon
Blue-green

43. Alkali metal compounds and NH4? compounds are...
Miscible with water - flammable - used as fuel - poisonous
21% of atmosphere - colorless - odorless - supports combustion reactions
Soluble
Involves water

44. Compounds with 12-18 carbons
Strong acids - strong bases - soluble salts
Two reactants combine to form a single product
Mixture of tin - copper - bismuth - and antimony
Make up jet fuels and kerosene

45. Octahedral
6 bonding - 90° - sp³d2² hybridization
Same element - different number of neutrons
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
8.3 to 10.0 - colorless to pink

46. Nitrate ion
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
NO3?
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
The solute is dissolved in the solvent.

47. Synthesis reaction
Two reactants combine to form a single product
Green
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Glass and plastic

48. What are the factors that affect reaction rate?
Mixture of tin - copper - bismuth - and antimony
CO3²?
M1V1 = M2V2
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

49. Aldehydes
DH = bonds broken - bonds formed
Classified as strong bases but not very soluble.
2 bonding - 180° - sp hybridization
COH functional group - name ends in -al

50. Solute vs. Solvent
Orange
5 bonding - 90° and 120° - sp³d hybridization
The solute is dissolved in the solvent.
Mixture of iron and carbon