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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. Ethanol
Etching glass and frosting lightblubs
Acid to water
DG = DH - TDS
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

2. Molarity
Magnesium
Moles / L
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Insoluble

3. Hydrogen gas properties
Gases at room temperature - used for fuel
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
21% of atmosphere - colorless - odorless - supports combustion reactions
Moles / L

4. Coal
6 bonding - 90° - sp³d2² hybridization
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Gas pressure = atm pressure + height of mercury
Covalent

5. Fission
3 bonding - 120° - sp² hybridization
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

6. bronze
Orange
Mixture of copper - zinc - and other metals
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

7. Suspension
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
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 compound breaks into two parts
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

8. Double replacement reaction
Stronger
Same formula - different structure
Two compound react to form two new compounds
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

9. Color of excited Na+
PV = nRT - R = .0821
Soluble
yellow
Etching glass and frosting lightblubs

10. What kind of bonds generally hold gases together?
3 bonding - 120° - sp² hybridization
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Moles / L
Covalent

11. Allotropic forms of carbon
Diamond - graphite - amorphous - fullerenes
Same molecule - different electron pair positions
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
No two electrons can have the same set of 4 quantum numbers

12. Solute vs. Solvent
The solute is dissolved in the solvent.
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Increase right and up
Yellow to orange

13. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
5 bonding - 90° and 120° - sp³d hybridization
NH4?
Soluble except when containing alkaline earth metals

14. Carboxylic acid group
COOH - ends in -oic acid
Gas pressure = atm pressure + height of mercury
Two atoms with the same number of electrons
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

15. Sulfide color: ZnS
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Bright yellow
White
6.0 to 7.6 - yellow to blue

16. Dilution equation
Q = mcDT
Mixture of tin - copper - bismuth - and antimony
M1V1 = M2V2
Lemon yellow

17. Acetate ion
Covalent
CO3²?
Mixture of tin - copper - bismuth - and antimony
C2H3O2?

18. Alkali Metals
1st group - most reactive metal family - react violently with water - create basic solutions
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Pressure of mixture of gases equals some of individual gas pressures.
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

19. Ammonium Ion
1st group - most reactive metal family - react violently with water - create basic solutions
NH4?
Yes
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

20. SO4²? compounds are...
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
Limited oxygen
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Properties of solutions that depend on the number of particles per solvent molecule

21. What kind of bonds generally hold liquids together?
PV = nRT - R = .0821
A compound breaks into two parts
Covalent
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

22. Color of Cu2+ solution
Blue
6.0 to 7.6 - yellow to blue
Glass and plastic
NH2 - ends in -amide

23. Compounds with 18 carbons
COOH - ends in -oic acid
Miscible with water - flammable - used as fuel - poisonous
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Solid at room temperature

24. What qualifies as a strong base?
Etching glass and frosting lightblubs
C2H3O2?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
SO4²?

25. Chlorine gas
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
OH - alcohols - name ends in ol
Heat required to make a substance melt.
Deadly - yellow-green - weapon

26. Carbonate ion
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
2 bonding - 180° - sp hybridization
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
CO3²?

27. Complete combustion occurs when there is
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Excess oxygen
Moles of solute / kg solvent
Yellow

28. Azimuthal quantum number (l)
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Defines shape of orbital
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

29. When the reaction is exothermic - the entropy is
COOH - ends in -oic acid
Miscible with water - flammable - used as fuel - poisonous
5 bonding - 90° and 120° - sp³d hybridization
Decreased

30. Oxygen gas properties
Orange
21% of atmosphere - colorless - odorless - supports combustion reactions
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

31. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Soluble except when containing Ag? - Hg2²? - or Pb²?
NH2 - ends in -amide
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

32. Nitrate ion
NO3?
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Electrons are free to move through metal structure - high conductivity - ductile
Classified as strong bases but not very soluble.

33. Color of MnO4? solution
Purple
Endothermic
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
It is at equilibrium

34. When a reaction is endothermic - the entropy is
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
The solute is dissolved in the solvent.
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Increased

35. Linear
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
2 bonding - 180° - sp hybridization
Pressure of mixture of gases equals some of individual gas pressures.
Same molecule - different electron pair positions

36. Sulfide color: CdS
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
White
Bright yellow
Do not conduct electricity well

37. Spin quantum number (ms)
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Spin is +1/2 or -1/2 in an orbital
Excess oxygen
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

38. Isoelectronic
Soluble
Two atoms with the same number of electrons
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

39. Phenolphthalein: pH range and colors
8.3 to 10.0 - colorless to pink
Yes in thermo - no in electro
Acid to water
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

40. Color of excited Li+ - Sr2+ - Ca2+
6.0 to 7.6 - yellow to blue
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Red
Gas pressure = atm pressure + height of mercury

41. Ketone
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
2 bonding - 1 nonbonding
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Solid at room temperature

42. London dispersion forces
Same element - different number of neutrons
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Classified as strong bases but not very soluble.
Soluble except when containing alkaline earth metals

43. Properties of ionic substances

44. Graham's Law
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
COOH functional group - name ends in oic acid
R-O-R functional group - shorter chain ends in oxy - other is ane
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

45. How can hydrogen be produced?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Strong acids - strong bases - soluble salts
Yellow

46. Ionization energy
Nonmetal oxides form acids - metal oxides form bases
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
NH2 - ends in -amide
DG = DH - TDS

47. Examples of strong electrolytes
Stronger
Involves water
Strong acids - strong bases - soluble salts
Deadly - yellow-green - weapon

48. Charles' Law
2 bonding - 180° - sp hybridization
Red
Endothermic
V1/T1 = V2/T2

49. What is the second law of thermodynamics?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Disordered systems with higher entropies are favored
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

50. Gibb's Free Energy equation
Mixture of copper - zinc - and other metals
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
DG = DH - TDS
3.1 - 4.4 - red to yellow