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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. Nonmetals
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Do not conduct electricity well
NH2 functional group - name ends in -amide

2. Complete combustion occurs when there is
Excess oxygen
3 bonding - 120° - sp² hybridization
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Gold

3. Fusion
Disordered systems with higher entropies are favored
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Gold
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

4. Molarity
DG = DH - TDS
NH2 - ends in -amide
Moles / L
R-O-R functional group - shorter chain ends in oxy - other is ane

5. Graham's Law
Lemon yellow
4 bonding - 109.5° - sp³ hybridization
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Two reactants combine to form a single product

6. What metal will react in hot water?
2 bonding - 180° - sp hybridization
Gases at room temperature - used for fuel
Magnesium
SO4²?

7. Add acid to water or water to acid
yellow
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
Acid to water
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

8. Alchohols
OH functional group - name ends in -ol
Two atoms with the same number of electrons
Blue
Mixture of iron and carbon

9. Charles' Law
NH2 functional group - name ends in -amide
Oxide that reacts with water to form either an acid or a base
It is at equilibrium
V1/T1 = V2/T2

10. Pi bonds
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Defines shape of orbital
Insoluble
Mixture of iron and carbon

11. Properties of acids
White
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
5 bonding - 90° and 120° - sp³d hybridization
Black

12. Acids with more oxygen atoms are
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Stronger
Mixture of copper and zinc
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

13. Color of Fe3+ solution
Moles / L
3 bonding - 1 nonbonding 107°
Yellow to orange
4.184

14. Magnetic quantum number (ml)
Liquid at room temperature - used to make gasoline and solvents
Strong acids - strong bases - soluble salts
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Orientation of orbital in space

15. Bromthymol blue: pH range and colors
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
6.0 to 7.6 - yellow to blue
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
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

16. Sulfide color: Sb2S3
Orange
Pressure of mixture of gases equals some of individual gas pressures.
Yellow to orange
Purple

17. Chlorine gas
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
4.5 to 8.3 - Red to blue
Deadly - yellow-green - weapon

18. Isomer
Diamond - graphite - amorphous - fullerenes
Same formula - different structure
Miscible with water - flammable - used as fuel - poisonous
OH functional group - name ends in -ol

19. Sulfide color: CuS - HgS - and PbS
Low pressures - high temperatures
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
8.3 to 10.0 - colorless to pink
Black

20. If G is zero - what is happening in the reaction?
Glass and plastic
Red
It is at equilibrium
Soluble except when containing Ag? - Hg2²? - or Pb²?

21. Boyle's Law
Limited oxygen
P1/V1 = P2/V2
1st group - most reactive metal family - react violently with water - create basic solutions
Etching glass and frosting lightblubs

22. Bent
Stronger
2 bonding - 1 nonbonding
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Potassium - Calcium - Sodium

23. Metallic bonds
Electrons are free to move through metal structure - high conductivity - ductile
Decreased
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

24. amphoteric
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
3.1 - 4.4 - red to yellow
Substance can act either as an acid or a base
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

25. Trigonal bipyramidal
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Solid at room temperature
5 bonding - 90° and 120° - sp³d hybridization
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

26. Alkali Metals
Stronger
1st group - most reactive metal family - react violently with water - create basic solutions
Limited oxygen
Covalent

27. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
NO3?
It is at equilibrium
Make up jet fuels and kerosene

28. Suspension
Purple/pink
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
C2H3O2?
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

29. If G is negative - is the reaction spontaneous?
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
V1/T1 = V2/T2
Yes
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

30. Exceptions to the octet rule
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Etching glass and frosting lightblubs
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
P1/V1 = P2/V2

31. Methyl orange: pH range and colors
3.1 - 4.4 - red to yellow
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
DG = DH - TDS

32. Color of Cu2+ solution
Blue
ClO3?
Yellow to orange
Orange

33. Gibb's Free Energy equation
Black
Do not conduct electricity well
DG = DH - TDS
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

34. When a reaction is endothermic - the entropy is
Periods 8 and 9 - lanthanides and actinides
Defines shape of orbital
Strong acids - strong bases - soluble salts
Increased

35. Hydrogen gas properties
Orange
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Photography
Glass and plastic

36. Noble gas properties
Photography
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Most stable

37. Sigma bonds
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
M1V1 = M2V2
Q = mcDT
No two electrons can have the same set of 4 quantum numbers

38. Linear
Etching glass and frosting lightblubs
4 bonding - 109.5° - sp³ hybridization
2 bonding - 180° - sp hybridization
Blue

39. Ester
Soluble except when containing alkaline earth metals
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Same formula - different structure

40. Amine group
Increases left and down
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
NH2 - ends in -amide
Diamond - graphite - amorphous - fullerenes

41. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Solid at room temperature
Soluble
No two electrons can have the same set of 4 quantum numbers
DG = DH - TDS

42. How many joules are in a calorie?
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Yes in thermo - no in electro
4.184
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

43. Beta particle
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Defines shape of orbital
COOH - ends in -oic acid

44. Fission
Magnesium
Light green
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
COH functional group - name ends in -al

45. Hydrofluoric acid is used for
Increase right and up
Etching glass and frosting lightblubs
Insoluble
Blue-green

46. Octahedral
Mixture of copper - zinc - and other metals
Two reactants combine to form a single product
6 bonding - 90° - sp³d2² hybridization
Etching glass and frosting lightblubs

47. Silver bromide and silver iodide are used for
Photography
Electrons are free to move through metal structure - high conductivity - ductile
Properties of solutions that depend on the number of particles per solvent molecule
Yellow to orange

48. bronze
Mixture of copper - zinc - and other metals
Covalent
OH - alcohols - name ends in ol
Mixture of silver and copper

49. Examples of amorphous solids
Energy level - as it increases electrons are less bound to the nucleus
Do not conduct electricity well
C2H3O2?
Glass and plastic

50. If G is positive - is the reaction spontaneous?
Stronger
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
No