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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. Boiling point elevation formula
More active element replaces less active element in a compound.
M1V1 = M2V2
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

2. Graham's Law
OH - alcohols - name ends in ol
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
More active element replaces less active element in a compound.
Orange

3. Charles' Law
Increases left and down
V1/T1 = V2/T2
Yellow to orange
6 bonding - 90° - sp³d2² hybridization

4. Positron emission
Soluble
Acid to water
Properties of solutions that depend on the number of particles per solvent molecule
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

5. What are the allotropic forms of sulfur?
Periods 8 and 9 - lanthanides and actinides
Electrons are free to move through metal structure - high conductivity - ductile
A compound breaks into two parts
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

6. 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.
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
No two electrons can have the same set of 4 quantum numbers
8.3 to 10.0 - colorless to pink

7. Allotropic forms of carbon
Mixture of silver and copper
Diamond - graphite - amorphous - fullerenes
Soluble
DH = bonds broken - bonds formed

8. Sulfide color: ZnS
White
Do not conduct electricity well
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Oxide that reacts with water to form either an acid or a base

9. Alpha particle
The solute is dissolved in the solvent.
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.
Limited oxygen
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

10. 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
Increase right and up
Degrade the oxone layer
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

11. Alkaline earth metals
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
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
2nd group - fairly reactive - pastes are used in batteries
ClO3?

12. Suspension
Purple/pink
P1/V1 = P2/V2
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
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

13. Color of Fe3+ solution
Same element - different number of neutrons
Yellow to orange
DH = bonds broken - bonds formed
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

14. Covalent bond
yellow
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.
Endothermic
Covalent

15. Sigma bonds
Defines shape of orbital
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

16. Ethers
3.1 - 4.4 - red to yellow
Photography
R-O-R functional group - shorter chain ends in oxy - other is ane
7th group - form salts - always exist as diatomic molecules - used in modern lighting

17. What kind of bonds generally hold liquids together?
Do not conduct electricity well
Covalent
6 bonding - 90° - sp³d2² hybridization
Increase right and up

18. Pi bonds
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
CO - produced from incomplete combustion - very toxic

19. How many joules are in a calorie?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
4.184
Moles of solute / kg solvent
Decreased

20. Ester
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Mixture of tin - copper - bismuth - and antimony
Substance can act either as an acid or a base

21. Color of excited Fe3+
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Extremely slow reactivity
Gold
Make up jet fuels and kerosene

22. What is the second law of thermodynamics?
Disordered systems with higher entropies are favored
Orientation of orbital in space
Gases at room temperature - used for fuel
4.184

23. Color of excited Ba2+
Stronger
Light green
Spin is +1/2 or -1/2 in an orbital
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

24. Compounds with 1-4 carbons
Gases at room temperature - used for fuel
Most stable
Diamond - graphite - amorphous - fullerenes
CO - produced from incomplete combustion - very toxic

25. Electronegativity
Covalent
Orientation of orbital in space
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Increase right and up

26. Cl - Br - and I compounds are...
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Yes in thermo - no in electro
Orientation of orbital in space
Soluble except when containing Ag? - Hg2²? - or Pb²?

27. Equation when using a barometer to calculate gas pressure.
Potassium - Calcium - Sodium
Substance can act either as an acid or a base
Gas pressure = atm pressure - height of mercury
CO3²?

28. Alchohols
OH functional group - name ends in -ol
2nd group - fairly reactive - pastes are used in batteries
Mixture of silver and copper
Orange

29. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Yes in thermo - no in electro
Gas pressure = atm pressure + height of mercury
6.0 to 7.6 - yellow to blue

30. Color of CrO7²? solution
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Q = mcDT
Orange
Light green

31. Sulfide color: CdS
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Bright yellow
6.0 to 7.6 - yellow to blue
Endothermic

32. Add acid to water or water to acid
Acid to water
Lemon yellow
PO4³?
It is at equilibrium

33. Gamma decay
Emission of electromagnetic energy after beta - positron - or alpha decay
Mixture of iron and carbon
NO3?
3 bonding - 1 nonbonding 107°

34. Decomposition reaction
COOH - ends in -oic acid
Oxide that reacts with water to form either an acid or a base
Stronger
A compound breaks into two parts

35. Incomplete combustion occurs when there is
Pressure of mixture of gases equals some of individual gas pressures.
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Limited oxygen
Same element - different number of neutrons

36. Molarity
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Moles / L
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

37. Acids with more oxygen atoms are
Nonmetal oxides form acids - metal oxides form bases
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
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
Stronger

38. List equivalent pressure values for mmHg - torr - atm - and Pa
Mixture of copper and zinc
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
C2H3O2?
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

39. What is the ideal gas law?
Etching glass and frosting lightblubs
Heat required to make a substance melt.
PV = nRT - R = .0821
Light green

40. Properties of acids
Electrons are free to move through metal structure - high conductivity - ductile
Soluble
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
Two reactants combine to form a single product

41. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Orange
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Etching glass and frosting lightblubs

42. Carboxylic acid
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
COOH functional group - name ends in oic acid
OH functional group - name ends in -ol
3 bonding - 1 nonbonding 107°

43. Complete combustion occurs when there is
Excess oxygen
Gas pressure = atm pressure + height of mercury
Red
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

44. Gibb's Free Energy equation
Orange
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
DG = DH - TDS

45. Compounds with 5-10 carbons
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Soluble
Liquid at room temperature - used to make gasoline and solvents

46. Litmus: pH range and colors
Extremely slow reactivity
4.5 to 8.3 - Red to blue
Blue-green
Soluble except when containing alkaline earth metals

47. Methanol
Miscible with water - flammable - used as fuel - poisonous
ClO3?
Covalent
Purple

48. Beta particle
Mixture of tin - copper - bismuth - and antimony
COOH - ends in -oic acid
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Solid at room temperature

49. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Soluble
White
Electrons are free to move through metal structure - high conductivity - ductile
Covalent

50. What is the equation used for heat transfer problems?
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Purple
Q = mcDT
Defines shape of orbital