Test your basic knowledge |

SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. When the reaction is exothermic - the entropy is
Yes in thermo - no in electro
2 bonding - 1 nonbonding
Decreased
2nd group - fairly reactive - pastes are used in batteries

2. Color of excited Cu2+
Blue-green
DH = bonds broken - bonds formed
Liquid at room temperature - used to make gasoline and solvents
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

3. Carboxylic acid
Properties of solutions that depend on the number of particles per solvent molecule
COOH functional group - name ends in oic acid
Two reactants combine to form a single product
Limited oxygen

4. Sulfide color: CuS - HgS - and PbS
Black
Energy level - as it increases electrons are less bound to the nucleus
Bright yellow
4.184

5. Sulfide color: ZnS
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.
Two atoms with the same number of electrons
White
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

6. Oxides are insoluble and when reacted with water..
Orientation of orbital in space
Nonmetal oxides form acids - metal oxides form bases
No
M1V1 = M2V2

7. General Properties of Organic Compounds
Black
PV = nRT - R = .0821
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

8. Bent
Purple/pink
Solid at room temperature
Orange
2 bonding - 1 nonbonding

9. Decomposition reaction
A compound breaks into two parts
Decreased
Increases left and down
Soluble

10. Noble gas properties
Photography
Most stable
yellow
Increased

11. Ethanol
Covalent
P1/V1 = P2/V2
8.3 to 10.0 - colorless to pink
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

12. Sulfide color: Sb2S3
Orange
Glass and plastic
Mixture of copper - zinc - and other metals
Electrons are free to move through metal structure - high conductivity - ductile

13. Dipole-dipole forces (including hydrogen bonds)
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Stronger
Electrons are free to move through metal structure - high conductivity - ductile

14. Color of CrO7²? solution
3 bonding - 120° - sp² hybridization
Orange
Blue-green
3 bonding - 1 nonbonding 107°

15. What are the allotropic forms of sulfur?
Diamond - graphite - amorphous - fullerenes
2 bonding - 1 nonbonding
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
M1V1 = M2V2

16. Dalton's Law
3 bonding - 120° - sp² hybridization
Pressure of mixture of gases equals some of individual gas pressures.
Increased
NH2 - ends in -amide

17. What is the equation used for heat transfer problems?
PO4³?
21% of atmosphere - colorless - odorless - supports combustion reactions
Q = mcDT
No

18. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Moles / L
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
NH2 - ends in -amide
Yes in thermo - no in electro

19. Sulfide color: As2S3
Insoluble
Do not conduct electricity well
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Lemon yellow

20. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Same formula - different structure
Blue
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

21. Ketone
Mixture of silver and copper
Heat required to make a substance melt.
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

22. Phenolphthalein: pH range and colors
No
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
8.3 to 10.0 - colorless to pink
Mixture of iron and carbon

23. Anhydride
Degrade the oxone layer
Oxide that reacts with water to form either an acid or a base
Purple
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

24. Hydrogen gas properties
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
NH2 functional group - name ends in -amide
Covalent

25. Metallic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
yellow
Gold

26. Halogen properties
yellow
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Diamond - graphite - amorphous - fullerenes

27. Gibb's Free Energy equation
COOH - ends in -oic acid
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
DG = DH - TDS
Properties of solutions that depend on the number of particles per solvent molecule

28. Charles' Law
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
It is at equilibrium
V1/T1 = V2/T2
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

29. Petroleum
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Low pressures - high temperatures
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

30. Molecular solids
2 bonding - 1 nonbonding
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Covalent
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

31. Bromthymol blue: pH range and colors
Soluble
2nd group - fairly reactive - pastes are used in batteries
6.0 to 7.6 - yellow to blue
Orientation of orbital in space

32. Noble gases
Extremely slow reactivity
Blue
Q = mcDT
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

33. Compounds with 12-18 carbons
Two atoms with the same number of electrons
Make up jet fuels and kerosene
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
OH functional group - name ends in -ol

34. Coal
Make up jet fuels and kerosene
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
Defines shape of orbital
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

35. Principal quantum number (n)
COOH - ends in -oic acid
C2H3O2?
Energy level - as it increases electrons are less bound to the nucleus
NO3?

36. Acids with more oxygen atoms are
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Q = mcDT
Stronger
NH2 - ends in -amide

37. Colloid
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
2 bonding - 1 nonbonding
Orange
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

38. What kind of bonds generally hold gases together?
R-O-R functional group - shorter chain ends in oxy - other is ane
Covalent
Same element - different number of neutrons
Green

39. Alchohols
Substance can act either as an acid or a base
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
OH functional group - name ends in -ol

40. Tetrahedral
4 bonding - 109.5° - sp³ hybridization
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
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
2 bonding - 180° - sp hybridization

41. Magnetic quantum number (ml)
Degrade the oxone layer
Increases left and down
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Orientation of orbital in space

42. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Etching glass and frosting lightblubs
Gas pressure = atm pressure + height of mercury
Two compound react to form two new compounds
White

43. Chlorate ion
COOH - ends in -oic acid
1st group - most reactive metal family - react violently with water - create basic solutions
ClO3?
Orientation of orbital in space

44. Colligative properties
Yes in thermo - no in electro
Electrons are free to move through metal structure - high conductivity - ductile
Two atoms with the same number of electrons
Properties of solutions that depend on the number of particles per solvent molecule

45. Carbon monoxide
Insoluble
Light green
CO - produced from incomplete combustion - very toxic
Classified as strong bases but not very soluble.

46. Octahedral
Black
6 bonding - 90° - sp³d2² hybridization
6.0 to 7.6 - yellow to blue
Bright yellow

47. Properties of bases
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Mixture of copper and zinc
Increases left and down

48. F compounds are...
Bright yellow
Mixture of silver and copper
Soluble except when containing alkaline earth metals
V1/T1 = V2/T2

49. Color of Fe3+ solution
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
It is at equilibrium
Yellow to orange

50. Covalent bond
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.
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
No two electrons can have the same set of 4 quantum numbers
OH - alcohols - name ends in ol