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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. Dipole-dipole forces (including hydrogen bonds)
Strong acids - strong bases - soluble salts
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
2nd group - fairly reactive - pastes are used in batteries
Yellow

2. Sulfide color: ZnS
PV = nRT - R = .0821
Diamond - graphite - amorphous - fullerenes
White
Mixture of copper - zinc - and other metals

3. Sulfide color: CdS
Most stable
NH2 - ends in -amide
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Bright yellow

4. What are the allotropic forms of sulfur?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Increased
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
CO3²?

5. Carbonate ion
Orange
Periods 8 and 9 - lanthanides and actinides
CO3²?
Mixture of tin - copper - bismuth - and antimony

6. Acids with more oxygen atoms are
Stronger
Defines shape of orbital
Photography
Strong acids - strong bases - soluble salts

7. Boiling point elevation formula
C2H3O2?
Light green
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

8. Sulfide color: As2S3
Lemon yellow
Gas pressure = atm pressure + height of mercury
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Yellow

9. Oxides are insoluble and when reacted with water..
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Gas pressure = atm pressure + height of mercury
Mixture of tin - copper - bismuth - and antimony
Nonmetal oxides form acids - metal oxides form bases

10. Add acid to water or water to acid
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
Acid to water
NO3?
Soluble except when containing alkaline earth metals

11. When the reaction is exothermic - the entropy is
Two reactants combine to form a single product
Decreased
It is at equilibrium
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

12. Ester
Glass and plastic
Heat required to make a substance melt.
White
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

13. List equivalent pressure values for mmHg - torr - atm - and Pa
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
ClO3?
It is at equilibrium
Extremely slow reactivity

14. Ammonium Ion
COH functional group - name ends in -al
Mixture of iron and carbon
Properties of solutions that depend on the number of particles per solvent molecule
NH4?

15. Ethanol
4.5 to 8.3 - Red to blue
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

16. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Mixture of iron and carbon
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

17. Covalent bond
Orange
White
Light green
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.

18. Sulfide color: Sb2S3
Moles / L
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
Orange
NH2 functional group - name ends in -amide

19. Sulfate ion
SO4²?
Light green
M1V1 = M2V2
Soluble except when containing alkaline earth metals

20. Molality
Soluble except when containing Ag? - Hg2²? - or Pb²?
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Moles of solute / kg solvent
Q = mcDT

21. Compounds with 5-10 carbons
Q = mcDT
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Liquid at room temperature - used to make gasoline and solvents
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

22. Ethers
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Nonmetal oxides form acids - metal oxides form bases
R-O-R functional group - shorter chain ends in oxy - other is ane
Bright yellow

23. Compounds with 12-18 carbons
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Make up jet fuels and kerosene
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Defines shape of orbital

24. Freezing point depression formula
Yes in thermo - no in electro
5 bonding - 90° and 120° - sp³d hybridization
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

25. Dilution equation
M1V1 = M2V2
Gold
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Orange

26. Methanol
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
V1/T1 = V2/T2
8.3 to 10.0 - colorless to pink
Miscible with water - flammable - used as fuel - poisonous

27. Ionic solids
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Substance can act either as an acid or a base
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
SO4²?

28. Gibb's Free Energy equation
C2H3O2?
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.
DG = DH - TDS
Orange

29. Cl - Br - and I compounds are...
Same element - different number of neutrons
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Soluble except when containing Ag? - Hg2²? - or Pb²?
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

30. Alkali metal properties
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Pressure of mixture of gases equals some of individual gas pressures.

31. Solute vs. Solvent
Green
Periods 8 and 9 - lanthanides and actinides
The solute is dissolved in the solvent.
Low pressures - high temperatures

32. Examples of strong electrolytes
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
SO4²?
Orientation of orbital in space
Strong acids - strong bases - soluble salts

33. Define heat of fusion.
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Heat required to make a substance melt.
Red
Covalent

34. Molarity
Liquid at room temperature - used to make gasoline and solvents
Etching glass and frosting lightblubs
Moles / L
Purple

35. Chlorate ion
Yes in thermo - no in electro
ClO3?
Soluble except when containing Ag? - Hg2²? - or Pb²?
Orientation of orbital in space

36. Color of CrO4²? solution
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Yellow
NH4?

37. Is removing an electron an exothermic or endothermic process?
Q = mcDT
Endothermic
PV = nRT - R = .0821
CO - produced from incomplete combustion - very toxic

38. Ionization energy
Liquid at room temperature - used to make gasoline and solvents
Low pressures - high temperatures
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
NH4?

39. Anhydride
M1V1 = M2V2
Oxide that reacts with water to form either an acid or a base
Degrade the oxone layer
Glass and plastic

40. Hydrofluoric acid is used for
3 bonding - 120° - sp² hybridization
Gas pressure = atm pressure + height of mercury
Etching glass and frosting lightblubs
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

41. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Soluble
Glass and plastic
OH - alcohols - name ends in ol
Mixture of copper - zinc - and other metals

42. Isoelectronic
Orientation of orbital in space
yellow
Light green
Two atoms with the same number of electrons

43. Colloid
Spin is +1/2 or -1/2 in an orbital
Excess oxygen
CO3²?
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

44. Compounds with 18 carbons
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Solid at room temperature
SO4²?

45. Alpha particle
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
4 bonding - 109.5° - sp³ hybridization
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
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

46. Properties of acids
Emission of electromagnetic energy after beta - positron - or alpha decay
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
Periods 8 and 9 - lanthanides and actinides
Strong acids - strong bases - soluble salts

47. General properties of alloys
2nd group - fairly reactive - pastes are used in batteries
Low pressures - high temperatures
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Increase right and up

48. Carbon dioxide gas properties
Low pressures - high temperatures
4 bonding - 109.5° - sp³ hybridization
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

49. Electron affinity
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Liquid at room temperature - used to make gasoline and solvents
Two reactants combine to form a single product
NH2 functional group - name ends in -amide

50. Oxygen gas properties
OH functional group - name ends in -ol
OH - alcohols - name ends in ol
21% of atmosphere - colorless - odorless - supports combustion reactions
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent