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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. Complete combustion occurs when there is
Red
Purple
Excess oxygen
Two atoms with the same number of electrons

2. Sulfide color: ZnS
White
More active element replaces less active element in a compound.
Solid at room temperature
Extremely slow reactivity

3. Hydrolysis reaction
Involves water
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
No
Decreased

4. Magnetic quantum number (ml)
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Orientation of orbital in space
Gas pressure = atm pressure - height of mercury
Oxide that reacts with water to form either an acid or a base

5. Oxides are insoluble and when reacted with water..
Covalent
1st group - most reactive metal family - react violently with water - create basic solutions
Magnesium
Nonmetal oxides form acids - metal oxides form bases

6. Suspension
3 bonding - 1 nonbonding 107°
Defines shape of orbital
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

7. What kind of bonds generally hold gases together?
PV = nRT - R = .0821
Blue-green
Covalent
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

8. Color of CrO4²? solution
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Same molecule - different electron pair positions
Liquid at room temperature - used to make gasoline and solvents
Yellow

9. Molecular solids
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Make up jet fuels and kerosene
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Lemon yellow

10. Phosphate ion
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Mixture of iron and carbon
PO4³?
Blue

11. What is the ideal gas law?
P1/V1 = P2/V2
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
PV = nRT - R = .0821

12. What are the factors that affect reaction rate?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
SO4²?
Green

13. Spin quantum number (ms)
More active element replaces less active element in a compound.
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Gases at room temperature - used for fuel
Spin is +1/2 or -1/2 in an orbital

14. Atomic radius trend
COOH functional group - name ends in oic acid
R-O-R functional group - shorter chain ends in oxy - other is ane
NH4?
Increases left and down

15. Bromthymol blue: pH range and colors
R-O-R functional group - shorter chain ends in oxy - other is ane
NO3?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
6.0 to 7.6 - yellow to blue

16. Compounds with 12-18 carbons
6 bonding - 90° - sp³d2² hybridization
No two electrons can have the same set of 4 quantum numbers
Make up jet fuels and kerosene
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

17. Sterling silver
Red
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
PO4³?
Mixture of silver and copper

18. Fission
PO4³?
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
NH2 functional group - name ends in -amide
Covalent

19. Steel
Do not conduct electricity well
Mixture of iron and carbon
7th group - form salts - always exist as diatomic molecules - used in modern lighting
NH2 - ends in -amide

20. General Properties of Organic Compounds
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Insoluble
Extremely slow reactivity

21. Properties of molecular crystals and liquids

22. Compounds with 1-4 carbons
Oxide that reacts with water to form either an acid or a base
Gases at room temperature - used for fuel
Disordered systems with higher entropies are favored
Involves water

23. Pi bonds
White
Gas pressure = atm pressure - height of mercury
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
A compound breaks into two parts

24. Sulfide color: CuS - HgS - and PbS
Black
Heat required to make a substance melt.
DH = bonds broken - bonds formed
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

25. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
Gas pressure = atm pressure + height of mercury
COOH functional group - name ends in oic acid
DH = bonds broken - bonds formed

26. Sulfide color: CdS
Covalent
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
Bright yellow
NH4?

27. Solute vs. Solvent
Mixture of copper and zinc
The solute is dissolved in the solvent.
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

28. Colloid
Degrade the oxone layer
2 bonding - 1 nonbonding
4.5 to 8.3 - Red to blue
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

29. Formula for calculating enthalpy change with bond energies
OH - alcohols - name ends in ol
Soluble
Soluble
DH = bonds broken - bonds formed

30. Metallic bonds
Electrons are free to move through metal structure - high conductivity - ductile
Excess oxygen
It is at equilibrium
Miscible with water - flammable - used as fuel - poisonous

31. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Soluble
Light green
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
R-O-R functional group - shorter chain ends in oxy - other is ane

32. Chlorofluorocarbons
Heat required to make a substance melt.
Lemon yellow
Degrade the oxone layer
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

33. What 3 metals will react with cold water?
Energy level - as it increases electrons are less bound to the nucleus
Mixture of silver and copper
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Potassium - Calcium - Sodium

34. Boyle's Law
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
6.0 to 7.6 - yellow to blue
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
P1/V1 = P2/V2

35. Is removing an electron an exothermic or endothermic process?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Deadly - yellow-green - weapon
Endothermic
Oxide that reacts with water to form either an acid or a base

36. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
It is at equilibrium
Etching glass and frosting lightblubs
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

37. Gibb's Free Energy equation
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
DG = DH - TDS
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

38. If G is negative - is the reaction spontaneous?
Magnesium
21% of atmosphere - colorless - odorless - supports combustion reactions
Low pressures - high temperatures
Yes

39. bronze
Energy level - as it increases electrons are less bound to the nucleus
Mixture of copper - zinc - and other metals
COOH - ends in -oic acid
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

40. Covalent-network / atomic solids
Orientation of orbital in space
Mixture of copper - zinc - and other metals
Pressure of mixture of gases equals some of individual gas pressures.
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

41. Carboxylic acid group
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
COOH - ends in -oic acid
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
6 bonding - 90° - sp³d2² hybridization

42. Ketone
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Heat required to make a substance melt.
OH - alcohols - name ends in ol
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

43. London dispersion forces
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
It is at equilibrium
Magnesium
PO4³?

44. Sulfate ion
SO4²?
Gas pressure = atm pressure + height of mercury
Magnesium
V1/T1 = V2/T2

45. Single Replacement / displacement reaction
M1V1 = M2V2
6 bonding - 90° - sp³d2² hybridization
More active element replaces less active element in a compound.
Low pressures - high temperatures

46. Amine
Periods 8 and 9 - lanthanides and actinides
Deadly - yellow-green - weapon
PV = nRT - R = .0821
NH2 functional group - name ends in -amide

47. Silver bromide and silver iodide are used for
Photography
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Decreased
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

48. Dilution equation
Magnesium
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
Do not conduct electricity well
M1V1 = M2V2

49. Beta particle
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
More active element replaces less active element in a compound.
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

50. Rare earth elements
Mixture of copper - zinc - and other metals
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Periods 8 and 9 - lanthanides and actinides
Purple/pink