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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. Color of Ni2+ solution
Green
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
SO4²?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

2. Halogen properties
3 bonding - 120° - sp² hybridization
SO4²?
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

3. 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.
Extremely slow reactivity
3 bonding - 120° - sp² hybridization
PV = nRT - R = .0821

4. What is the second law of thermodynamics?
Disordered systems with higher entropies are favored
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Gold
Orange

5. Aldehydes
COH functional group - name ends in -al
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Stronger
Substance can act either as an acid or a base

6. Magnetic quantum number (ml)
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
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Orientation of orbital in space
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

7. Acetate ion
NH2 - ends in -amide
2 bonding - 180° - sp hybridization
C2H3O2?
Energy level - as it increases electrons are less bound to the nucleus

8. Freezing point depression formula
COOH - ends in -oic acid
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Decreased
Diamond - graphite - amorphous - fullerenes

9. Atomic radius trend
Increases left and down
Yellow
2nd group - fairly reactive - pastes are used in batteries
Increased

10. Synthesis reaction
Properties of solutions that depend on the number of particles per solvent molecule
Miscible with water - flammable - used as fuel - poisonous
Energy level - as it increases electrons are less bound to the nucleus
Two reactants combine to form a single product

11. Amine
Properties of solutions that depend on the number of particles per solvent molecule
Yellow to orange
NH2 functional group - name ends in -amide
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

12. Equation when using a barometer to calculate gas pressure.
Moles / L
Involves water
DG = DH - TDS
Gas pressure = atm pressure - height of mercury

13. Pi bonds
Gold
Insoluble
OH functional group - name ends in -ol
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

14. Dalton's Law
White
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Pressure of mixture of gases equals some of individual gas pressures.
Increases left and down

15. Compounds with 12-18 carbons
Make up jet fuels and kerosene
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Gold
SO4²?

16. Double replacement reaction
DG = DH - TDS
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
Miscible with water - flammable - used as fuel - poisonous
Two compound react to form two new compounds

17. Color of CrO4²? solution
Properties of solutions that depend on the number of particles per solvent molecule
Yellow
2 bonding - 180° - sp hybridization
More active element replaces less active element in a compound.

18. Fission
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Two compound react to form two new compounds
ClO3?

19. Color of Cu2+ solution
Orange
NH4?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Blue

20. Examples of strong electrolytes
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
Covalent
Strong acids - strong bases - soluble salts
Yellow

21. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Disordered systems with higher entropies are favored
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Insoluble
Strong acids - strong bases - soluble salts

22. Sulfide color: CdS
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Bright yellow
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
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

23. Colloid
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
2nd group - fairly reactive - pastes are used in batteries
PV = nRT - R = .0821
Soluble

24. Carbon dioxide gas properties
Orange
Make up jet fuels and kerosene
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Moles of solute / kg solvent

25. Isotope
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Classified as strong bases but not very soluble.
Same element - different number of neutrons
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

26. Hydrogen gas properties
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Yellow to orange
ClO3?
Same element - different number of neutrons

27. Bent
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
2 bonding - 1 nonbonding
SO4²?
Moles / L

28. London dispersion forces
Black
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Two compound react to form two new compounds
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

29. Properties of bases
Orientation of orbital in space
A compound breaks into two parts
Soluble except when containing Ag? - Hg2²? - or Pb²?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

30. Chlorine gas
Deadly - yellow-green - weapon
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
2 bonding - 180° - sp hybridization
M1V1 = M2V2

31. Litmus: pH range and colors
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Emission of electromagnetic energy after beta - positron - or alpha decay
NH2 - ends in -amide
4.5 to 8.3 - Red to blue

32. Carbonate ion
Strong acids - strong bases - soluble salts
PV = nRT - R = .0821
8.3 to 10.0 - colorless to pink
CO3²?

33. Hydrofluoric acid is used for
Yellow
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Etching glass and frosting lightblubs
V1/T1 = V2/T2

34. Tetrahedral
Disordered systems with higher entropies are favored
Diamond - graphite - amorphous - fullerenes
4 bonding - 109.5° - sp³ hybridization
Heat required to make a substance melt.

35. Beta particle
R-O-R functional group - shorter chain ends in oxy - other is ane
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
6 bonding - 90° - sp³d2² hybridization
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

36. Sulfide color: As2S3
Energy level - as it increases electrons are less bound to the nucleus
COOH - ends in -oic acid
Endothermic
Lemon yellow

37. Ester
Blue-green
Etching glass and frosting lightblubs
White
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

38. Nonmetals
Do not conduct electricity well
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
P1/V1 = P2/V2
Solid at room temperature

39. When a reaction is endothermic - the entropy is
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Etching glass and frosting lightblubs
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Increased

40. Supersaturated solution
It is at equilibrium
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Same molecule - different electron pair positions
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

41. Radioactivity
Insoluble
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Substance can act either as an acid or a base
Decreased

42. Gamma decay
Heat required to make a substance melt.
4.184
Emission of electromagnetic energy after beta - positron - or alpha decay
SO4²?

43. F compounds are...
No two electrons can have the same set of 4 quantum numbers
2 bonding - 180° - sp hybridization
Purple/pink
Soluble except when containing alkaline earth metals

44. 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
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.
2 bonding - 1 nonbonding
8.3 to 10.0 - colorless to pink

45. Phosphate ion
Spin is +1/2 or -1/2 in an orbital
PO4³?
Diamond - graphite - amorphous - fullerenes
4 bonding - 109.5° - sp³ hybridization

46. Alkaline metal oxides are...
Decreased
Strong acids - strong bases - soluble salts
Classified as strong bases but not very soluble.
OH functional group - name ends in -ol

47. Ammonium Ion
NH4?
Orange
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Emission of electromagnetic energy after beta - positron - or alpha decay

48. Alchohols
Yes
2 bonding - 1 nonbonding
Yes in thermo - no in electro
OH functional group - name ends in -ol

49. Metallic bonds
Electrons are free to move through metal structure - high conductivity - ductile
Orange
Involves water
Magnesium

50. Boyle's Law
P1/V1 = P2/V2
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Disordered systems with higher entropies are favored
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl