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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. Color of excited K+
Purple/pink
Orientation of orbital in space
ClO3?
NH2 functional group - name ends in -amide

2. Solute vs. Solvent
Moles of solute / kg solvent
The solute is dissolved in the solvent.
Miscible with water - flammable - used as fuel - poisonous
Make up jet fuels and kerosene

3. Ethers
R-O-R functional group - shorter chain ends in oxy - other is ane
V1/T1 = V2/T2
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
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

4. Alkaline metal oxides are...
No
Classified as strong bases but not very soluble.
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

5. What metal will react in hot water?
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
Etching glass and frosting lightblubs
Magnesium
M1V1 = M2V2

6. Ionic solids
Covalent
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
C2H3O2?
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

7. Ester
Light green
COOH - ends in -oic acid
Spin is +1/2 or -1/2 in an orbital
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

8. Color of Cu2+ solution
Blue
Orange
3 bonding - 1 nonbonding 107°
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

9. Compounds with 1-4 carbons
Degrade the oxone layer
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
Gases at room temperature - used for fuel
Liquid at room temperature - used to make gasoline and solvents

10. Synthesis reaction
Two reactants combine to form a single product
Emission of electromagnetic energy after beta - positron - or alpha decay
Pressure of mixture of gases equals some of individual gas pressures.
Magnesium

11. What is the equation used for heat transfer problems?
PO4³?
Q = mcDT
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

12. Alpha particle
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
Properties of solutions that depend on the number of particles per solvent molecule
Heat required to make a substance melt.
Increased

13. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Soluble
Mixture of iron and carbon
Gas pressure = atm pressure + height of mercury
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

14. Dipole-dipole forces (including hydrogen bonds)
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Insoluble
P1/V1 = P2/V2

15. Carbon dioxide gas properties
DG = DH - TDS
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Yellow
Stronger

16. Radioactivity
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Q = mcDT
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Involves water

17. Complete combustion occurs when there is
Excess oxygen
Blue-green
Mixture of tin - copper - bismuth - and antimony
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

18. Equation when using a barometer to calculate gas pressure.
Gas pressure = atm pressure - height of mercury
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
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.
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

19. Beta particle
7th group - form salts - always exist as diatomic molecules - used in modern lighting
1. don't conduct good current 2. many exist as gases at room temp 3. melting points of solid crystals are low 4. large amount of energy needed to decompose
Red
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

20. Molarity
Low pressures - high temperatures
Moles / L
Same element - different number of neutrons
Mixture of tin - copper - bismuth - and antimony

21. Tetrahedral
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Purple/pink
4 bonding - 109.5° - sp³ hybridization
Heat required to make a substance melt.

22. Boiling point elevation formula
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Most stable
Mixture of copper - zinc - and other metals
M1V1 = M2V2

23. What 3 metals will react with cold water?
Decreased
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Potassium - Calcium - Sodium
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

24. Pauli exclusion principle
NO3?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Gas pressure = atm pressure + height of mercury
No two electrons can have the same set of 4 quantum numbers

25. Carbon monoxide
Deadly - yellow-green - weapon
R-O-R functional group - shorter chain ends in oxy - other is ane
CO - produced from incomplete combustion - very toxic
Glass and plastic

26. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Degrade the oxone layer
6.0 to 7.6 - yellow to blue
Gas pressure = atm pressure + height of mercury

27. Fusion
Gas pressure = atm pressure + height of mercury
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Do not conduct electricity well
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

28. Nonmetals
Purple
Two compound react to form two new compounds
2 bonding - 1 nonbonding
Do not conduct electricity well

29. Amine
Magnesium
P1/V1 = P2/V2
NH2 functional group - name ends in -amide
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

30. Acids with more oxygen atoms are
M1V1 = M2V2
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Soluble except when containing alkaline earth metals
Stronger

31. Hydrofluoric acid is used for
DH = bonds broken - bonds formed
Etching glass and frosting lightblubs
ClO3?
Make up jet fuels and kerosene

32. When a reaction is endothermic - the entropy is
Properties of solutions that depend on the number of particles per solvent molecule
Solid at room temperature
Increased
4 bonding - 109.5° - sp³ hybridization

33. Linear
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Purple/pink
Orientation of orbital in space
2 bonding - 180° - sp hybridization

34. Alkali metal compounds and NH4? compounds are...
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.
Soluble
3 bonding - 120° - sp² hybridization
Deadly - yellow-green - weapon

35. Hydroxyl group
OH - alcohols - name ends in ol
P1/V1 = P2/V2
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Mixture of copper - zinc - and other metals

36. Aldehydes
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
COH functional group - name ends in -al
Yellow
R-O-R functional group - shorter chain ends in oxy - other is ane

37. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
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.
Soluble

38. Properties of bases
Deadly - yellow-green - weapon
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
PO4³?
Blue

39. When the reaction is exothermic - the entropy is
Decreased
Gas pressure = atm pressure + height of mercury
Most stable
Increase right and up

40. Sulfide color: As2S3
Lemon yellow
Same formula - different structure
Strong acids - strong bases - soluble salts
2nd group - fairly reactive - pastes are used in batteries

41. Carboxylic acid group
Soluble except when containing alkaline earth metals
Low pressures - high temperatures
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
COOH - ends in -oic acid

42. bronze
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Excess oxygen
COH functional group - name ends in -al
Mixture of copper - zinc - and other metals

43. Colloid
Covalent
SO4²?
Substance can act either as an acid or a base
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

44. Add acid to water or water to acid
Black
Acid to water
OH functional group - name ends in -ol
Magnesium

45. Ammonium Ion
Gold
NH4?
Moles / L
yellow

46. Suspension
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
5 bonding - 90° and 120° - sp³d hybridization
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

47. Color of Ni2+ solution
Decreased
Etching glass and frosting lightblubs
Green
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

48. What kind of bonds generally hold liquids together?
Covalent
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Red
Blue

49. Properties of molecular crystals and liquids

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50. Incomplete combustion occurs when there is
Electrons are free to move through metal structure - high conductivity - ductile
Limited oxygen
Decreased
White