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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. Chlorine gas
Deadly - yellow-green - weapon
Orange
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
P1/V1 = P2/V2

2. Define heat of fusion.
Heat required to make a substance melt.
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
Substance can act either as an acid or a base
3.1 - 4.4 - red to yellow

3. Decomposition reaction
A compound breaks into two parts
1st group - most reactive metal family - react violently with water - create basic solutions
Mixture of copper and zinc
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

4. Allotropic forms of carbon
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Diamond - graphite - amorphous - fullerenes
Electrons are free to move through metal structure - high conductivity - ductile
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

5. Sterling silver
Potassium - Calcium - Sodium
SO4²?
Mixture of silver and copper
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

6. Ethanol
C2H3O2?
Increases left and down
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

7. Color of excited Li+ - Sr2+ - Ca2+
Red
Yes
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Orientation of orbital in space

8. Suspension
Orientation of orbital in space
CO - produced from incomplete combustion - very toxic
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Energy level - as it increases electrons are less bound to the nucleus

9. Sulfide color: CuS - HgS - and PbS
Gold
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
NH2 - ends in -amide
Black

10. Bent
2 bonding - 1 nonbonding
Substance can act either as an acid or a base
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Mixture of silver and copper

11. Carbonate ion
Stronger
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
CO3²?

12. Properties of bases
Involves water
Yellow
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

13. Cl - Br - and I compounds are...
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Soluble except when containing Ag? - Hg2²? - or Pb²?
Classified as strong bases but not very soluble.

14. Sulfate ion
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
yellow
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
SO4²?

15. Phosphate ion
Decreased
6 bonding - 90° - sp³d2² hybridization
PO4³?
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

16. Ionization energy
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
DH = bonds broken - bonds formed
CO3²?

17. When a reaction is endothermic - the entropy is
Degrade the oxone layer
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Increased
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

18. What is the ideal gas law?
PV = nRT - R = .0821
Soluble
Limited oxygen
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

19. Color of excited Na+
Defines shape of orbital
Increased
yellow
V1/T1 = V2/T2

20. Colligative properties
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Gases at room temperature - used for fuel
Properties of solutions that depend on the number of particles per solvent molecule
Purple

21. Ionic bond
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
Mixture of copper - zinc - and other metals
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

22. Azimuthal quantum number (l)
Defines shape of orbital
Solid at room temperature
Light green
2 bonding - 1 nonbonding

23. Alkali metal properties
NH2 functional group - name ends in -amide
M1V1 = M2V2
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

24. Colloid
C2H3O2?
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Yellow
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

25. Chlorofluorocarbons
Strong acids - strong bases - soluble salts
Degrade the oxone layer
M1V1 = M2V2
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

26. Color of Fe3+ solution
Covalent
Yellow to orange
Increase right and up
Lemon yellow

27. Examples of amorphous solids
Glass and plastic
Lemon yellow
Strong acids - strong bases - soluble salts
No

28. What kind of bonds generally hold liquids together?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
A compound breaks into two parts
Covalent

29. Metallic bonds
Gold
Miscible with water - flammable - used as fuel - poisonous
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

30. Alchohols
4.184
OH functional group - name ends in -ol
DG = DH - TDS
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

31. If G is positive - is the reaction spontaneous?
Extremely slow reactivity
Mixture of copper and zinc
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
No

32. Amine
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
NH2 functional group - name ends in -amide
Disordered systems with higher entropies are favored
A compound breaks into two parts

33. If G is zero - what is happening in the reaction?
It is at equilibrium
PO4³?
Energy level - as it increases electrons are less bound to the nucleus
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

34. Tetrahedral
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
4 bonding - 109.5° - sp³ hybridization
Oxide that reacts with water to form either an acid or a base
C2H3O2?

35. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
3 bonding - 120° - sp² hybridization
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Acid to water

36. Gibb's Free Energy equation
M1V1 = M2V2
DG = DH - TDS
More active element replaces less active element in a compound.
Strong acids - strong bases - soluble salts

37. Anhydride
NH4?
PO4³?
No two electrons can have the same set of 4 quantum numbers
Oxide that reacts with water to form either an acid or a base

38. What are the factors that affect reaction rate?
A compound breaks into two parts
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

39. Properties of ionic substances

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40. Methanol
CO - produced from incomplete combustion - very toxic
Miscible with water - flammable - used as fuel - poisonous
Solid at room temperature
CO3²?

41. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
NH2 - ends in -amide
2 bonding - 1 nonbonding
Covalent

42. amphoteric
COOH - ends in -oic acid
Substance can act either as an acid or a base
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

43. Alkali metal compounds and NH4? compounds are...
Moles / L
Soluble
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
R-O-R functional group - shorter chain ends in oxy - other is ane

44. Incomplete combustion occurs when there is
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Limited oxygen
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

45. Combustion reaction
SO4²?
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Same formula - different structure
White

46. Charles' Law
Yellow
NH4?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
V1/T1 = V2/T2

47. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
ClO3?
Degrade the oxone layer

48. Compounds with 5-10 carbons
Soluble except when containing alkaline earth metals
4 bonding - 109.5° - sp³ hybridization
Liquid at room temperature - used to make gasoline and solvents
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

49. Molarity
Two reactants combine to form a single product
Covalent
Two compound react to form two new compounds
Moles / L

50. Covalent bond
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.
Orange
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
OH functional group - name ends in -ol