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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. How many joules are in a calorie?
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Mixture of silver and copper
4.184
ClO3?

2. Ester
3 bonding - 1 nonbonding 107°
Blue
Mixture of copper - zinc - and other metals
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

3. Brass
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
DH = bonds broken - bonds formed
Substance can act either as an acid or a base
Mixture of copper and zinc

4. Fission
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Green
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Gases at room temperature - used for fuel

5. Petroleum
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
Moles / L
Nonmetal oxides form acids - metal oxides form bases

6. Color of CrO4²? solution
Q = mcDT
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Yellow
Mixture of silver and copper

7. Methyl orange: pH range and colors
Gases at room temperature - used for fuel
Soluble except when containing Ag? - Hg2²? - or Pb²?
3.1 - 4.4 - red to yellow
PV = nRT - R = .0821

8. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Two compound react to form two new compounds
Insoluble
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
Yellow to orange

9. Dipole-dipole forces (including hydrogen bonds)
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Same element - different number of neutrons
NH2 functional group - name ends in -amide

10. Resonance structures
Black
Electrons are free to move through metal structure - high conductivity - ductile
Same molecule - different electron pair positions
Two reactants combine to form a single product

11. Carbon monoxide
No two electrons can have the same set of 4 quantum numbers
Miscible with water - flammable - used as fuel - poisonous
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
CO - produced from incomplete combustion - very toxic

12. What is the second law of thermodynamics?
Liquid at room temperature - used to make gasoline and solvents
Low pressures - high temperatures
Disordered systems with higher entropies are favored
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

13. Tetrahedral
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
4 bonding - 109.5° - sp³ hybridization
Yes in thermo - no in electro
Periods 8 and 9 - lanthanides and actinides

14. Sterling silver
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
V1/T1 = V2/T2
Mixture of silver and copper

15. Alkali Metals
1st group - most reactive metal family - react violently with water - create basic solutions
Light green
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
4 bonding - 109.5° - sp³ hybridization

16. Bromthymol blue: pH range and colors
Etching glass and frosting lightblubs
6.0 to 7.6 - yellow to blue
Emission of electromagnetic energy after beta - positron - or alpha decay
PV = nRT - R = .0821

17. What 3 metals will react with cold water?
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Endothermic
Potassium - Calcium - Sodium

18. Ionic solids
Degrade the oxone layer
Light green
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Emission of electromagnetic energy after beta - positron - or alpha decay

19. What is the ideal gas law?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Moles / L
PV = nRT - R = .0821
Properties of solutions that depend on the number of particles per solvent molecule

20. Fusion
Soluble
2 bonding - 1 nonbonding
Pressure of mixture of gases equals some of individual gas pressures.
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

21. Carboxylic acid group
NH2 - ends in -amide
3.1 - 4.4 - red to yellow
COOH - ends in -oic acid
Purple/pink

22. Solute vs. Solvent
The solute is dissolved in the solvent.
COH functional group - name ends in -al
COOH functional group - name ends in oic acid
Degrade the oxone layer

23. Aldehydes
COH functional group - name ends in -al
yellow
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Heat required to make a substance melt.

24. Molarity
Acid to water
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
Moles / L
Covalent

25. Chlorine gas
More active element replaces less active element in a compound.
Yes
Deadly - yellow-green - weapon
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

26. Ammonium Ion
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
NH4?
Endothermic
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

27. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
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
Blue
7th group - form salts - always exist as diatomic molecules - used in modern lighting

28. Gibb's Free Energy equation
PV = nRT - R = .0821
DG = DH - TDS
21% of atmosphere - colorless - odorless - supports combustion reactions
Yes

29. Rare earth elements
Periods 8 and 9 - lanthanides and actinides
Black
Properties of solutions that depend on the number of particles per solvent molecule
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

30. SO4²? compounds are...
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Electrons are free to move through metal structure - high conductivity - ductile
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

31. Synthesis reaction
Two reactants combine to form a single product
Mixture of copper - zinc - and other metals
COH functional group - name ends in -al
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

32. Metallic solids
Potassium - Calcium - Sodium
Properties of solutions that depend on the number of particles per solvent molecule
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Electrons are free to move through metal structure - high conductivity - ductile

33. Atomic radius trend
4.184
More active element replaces less active element in a compound.
Increases left and down
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

34. Gamma decay
Orange
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Mixture of tin - copper - bismuth - and antimony
Emission of electromagnetic energy after beta - positron - or alpha decay

35. Electronegativity
Increase right and up
Classified as strong bases but not very soluble.
6.0 to 7.6 - yellow to blue
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

36. Properties of acids
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Low pressures - high temperatures
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
A compound breaks into two parts

37. Radioactivity
Solid at room temperature
Substance can act either as an acid or a base
Black
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

38. Methanol
Miscible with water - flammable - used as fuel - poisonous
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Increases left and down
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

39. Colloid
Black
It is at equilibrium
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
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

40. Compounds with 12-18 carbons
Stronger
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
3.1 - 4.4 - red to yellow
Make up jet fuels and kerosene

41. Dilution equation
It is at equilibrium
2 bonding - 180° - sp hybridization
Soluble
M1V1 = M2V2

42. Sulfide color: ZnS
Covalent
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
M1V1 = M2V2
White

43. General properties of alloys
C2H3O2?
PO4³?
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Mixture of iron and carbon

44. Decomposition reaction
Yes
A compound breaks into two parts
No two electrons can have the same set of 4 quantum numbers
Strong acids - strong bases - soluble salts

45. Compounds with 18 carbons
Gas pressure = atm pressure + height of mercury
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Pressure of mixture of gases equals some of individual gas pressures.
Solid at room temperature

46. Acetate ion
3.1 - 4.4 - red to yellow
C2H3O2?
Etching glass and frosting lightblubs
Purple

47. Hydrofluoric acid is used for
NH2 functional group - name ends in -amide
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Etching glass and frosting lightblubs
Gas pressure = atm pressure + height of mercury

48. Transition metals
Green
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Same element - different number of neutrons
Same formula - different structure

49. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Periods 8 and 9 - lanthanides and actinides
Green
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Soluble

50. Compounds with 5-10 carbons
NH2 functional group - name ends in -amide
Blue
Liquid at room temperature - used to make gasoline and solvents
Electrons are free to move through metal structure - high conductivity - ductile