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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. Alkaline metal oxides are...
Classified as strong bases but not very soluble.
Orange
No
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

2. Hydrolysis reaction
Involves water
No two electrons can have the same set of 4 quantum numbers
Moles / L
Yes

3. 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
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Acid to water
Same element - different number of neutrons

4. Noble gas properties
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
DH = bonds broken - bonds formed
Gas pressure = atm pressure + height of mercury
Most stable

5. Resonance structures
Degrade the oxone layer
Same molecule - different electron pair positions
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Soluble except when containing Ag? - Hg2²? - or Pb²?

6. Pi bonds
Nonmetal oxides form acids - metal oxides form bases
Yes in thermo - no in electro
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Lemon yellow

7. Ammonium Ion
PV = nRT - R = .0821
NH4?
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Soluble

8. Trigonal pyramidal
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
No two electrons can have the same set of 4 quantum numbers
3 bonding - 1 nonbonding 107°
ClO3?

9. Examples of strong electrolytes
Strong acids - strong bases - soluble salts
Soluble except when containing alkaline earth metals
OH - alcohols - name ends in ol
Increased

10. Color of excited Cu2+
Blue-green
Insoluble
Increase right and up
Lemon yellow

11. Double replacement reaction
Substance can act either as an acid or a base
Two compound react to form two new compounds
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
21% of atmosphere - colorless - odorless - supports combustion reactions

12. Methanol
Increases left and down
Photography
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Miscible with water - flammable - used as fuel - poisonous

13. Ionic bond
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Covalent
2 bonding - 1 nonbonding
Do not conduct electricity well

14. Graham's Law
Endothermic
It is at equilibrium
Most stable
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

15. Nonmetals
Do not conduct electricity well
yellow
8.3 to 10.0 - colorless to pink
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

16. Charles' Law
Disordered systems with higher entropies are favored
5 bonding - 90° and 120° - sp³d hybridization
Soluble
V1/T1 = V2/T2

17. Octahedral
6 bonding - 90° - sp³d2² hybridization
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Involves water

18. When are gases MOST ideal?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
2nd group - fairly reactive - pastes are used in batteries
Low pressures - high temperatures
Emission of electromagnetic energy after beta - positron - or alpha decay

19. Properties of bases
Classified as strong bases but not very soluble.
Pressure of mixture of gases equals some of individual gas pressures.
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
NH4?

20. Gibb's Free Energy equation
Soluble
DG = DH - TDS
Covalent
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

21. Decomposition reaction
6 bonding - 90° - sp³d2² hybridization
CO - produced from incomplete combustion - very toxic
A compound breaks into two parts
Nonmetal oxides form acids - metal oxides form bases

22. Compounds with 12-18 carbons
Mixture of iron and carbon
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Make up jet fuels and kerosene
yellow

23. Alkali metal compounds and NH4? compounds are...
Soluble
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Purple
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

24. amphoteric
Acid to water
Gold
Substance can act either as an acid or a base
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

25. Carbon dioxide gas properties
Glass and plastic
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
The solute is dissolved in the solvent.
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

26. Ester
Purple
Increase right and up
Increases left and down
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

27. Trigonal bipyramidal
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Excess oxygen
5 bonding - 90° and 120° - sp³d hybridization
More active element replaces less active element in a compound.

28. Chlorine gas
Potassium - Calcium - Sodium
C2H3O2?
Deadly - yellow-green - weapon
Same molecule - different electron pair positions

29. Freezing point depression formula
Make up jet fuels and kerosene
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Strong acids - strong bases - soluble salts
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

30. Sulfide color: As2S3
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
5 bonding - 90° and 120° - sp³d hybridization
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
Lemon yellow

31. Ethers
Etching glass and frosting lightblubs
Degrade the oxone layer
PO4³?
R-O-R functional group - shorter chain ends in oxy - other is ane

32. Carbonate ion
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
CO3²?
Low pressures - high temperatures
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

33. What is the second law of thermodynamics?
COOH - ends in -oic acid
Mixture of tin - copper - bismuth - and antimony
Disordered systems with higher entropies are favored
Gold

34. Equation when using a barometer to calculate gas pressure.
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Diamond - graphite - amorphous - fullerenes
Gas pressure = atm pressure - height of mercury
Gold

35. Boiling point elevation formula
Mixture of tin - copper - bismuth - and antimony
Energy level - as it increases electrons are less bound to the nucleus
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

36. When a reaction is endothermic - the entropy is
NH2 functional group - name ends in -amide
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
R-O-R functional group - shorter chain ends in oxy - other is ane
Increased

37. Suspension
Soluble except when containing alkaline earth metals
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

38. Pauli exclusion principle
No two electrons can have the same set of 4 quantum numbers
DH = bonds broken - bonds formed
yellow
Increased

39. Colligative properties
Mixture of tin - copper - bismuth - and antimony
NH2 - ends in -amide
COH functional group - name ends in -al
Properties of solutions that depend on the number of particles per solvent molecule

40. Color of CrO4²? solution
5 bonding - 90° and 120° - sp³d hybridization
Blue-green
Yellow
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

41. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Most stable
Two atoms with the same number of electrons
Energy level - as it increases electrons are less bound to the nucleus

42. Is removing an electron an exothermic or endothermic process?
Acid to water
Endothermic
C2H3O2?
Defines shape of orbital

43. Halogens
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Yellow to orange
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Do not conduct electricity well

44. Add acid to water or water to acid
Potassium - Calcium - Sodium
Excess oxygen
Acid to water
Same molecule - different electron pair positions

45. Formula for calculating enthalpy change with bond energies
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
6 bonding - 90° - sp³d2² hybridization
DH = bonds broken - bonds formed
Increased

46. Complete combustion occurs when there is
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
SO4²?
Excess oxygen
3 bonding - 120° - sp² hybridization

47. Tetrahedral
6 bonding - 90° - sp³d2² hybridization
Classified as strong bases but not very soluble.
Increased
4 bonding - 109.5° - sp³ hybridization

48. Properties of molecular crystals and liquids

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49. Linear
Liquid at room temperature - used to make gasoline and solvents
Yellow
Blue
2 bonding - 180° - sp hybridization

50. Principal quantum number (n)
Same formula - different structure
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Energy level - as it increases electrons are less bound to the nucleus
Endothermic