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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. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Mixture of iron and carbon
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

2. Decomposition reaction
COH functional group - name ends in -al
Q = mcDT
A compound breaks into two parts
Oxide that reacts with water to form either an acid or a base

3. Equation when using a barometer to calculate gas pressure.
Red
Gas pressure = atm pressure - height of mercury
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Decreased

4. Pi bonds
OH - alcohols - name ends in ol
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.
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Two compound react to form two new compounds

5. Properties of bases
Heat required to make a substance melt.
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Purple
NH2 - ends in -amide

6. Trigonal pyramidal
Periods 8 and 9 - lanthanides and actinides
3 bonding - 1 nonbonding 107°
Bright yellow
Involves water

7. Principal quantum number (n)
Energy level - as it increases electrons are less bound to the nucleus
Gas pressure = atm pressure + height of mercury
More active element replaces less active element in a compound.
Oxide that reacts with water to form either an acid or a base

8. Sulfate ion
SO4²?
Red
Periods 8 and 9 - lanthanides and actinides
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

9. Add acid to water or water to acid
Most stable
Mixture of iron and carbon
Acid to water
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

10. Magnetic quantum number (ml)
Orientation of orbital in space
Increases left and down
Yes in thermo - no in electro
Two atoms with the same number of electrons

11. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Gas pressure = atm pressure + height of mercury
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
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.

12. Atomic radius trend
The solute is dissolved in the solvent.
ClO3?
Increases left and down
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

13. 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
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
ClO3?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

14. Hydrofluoric acid is used for
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
P1/V1 = P2/V2
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Etching glass and frosting lightblubs

15. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
Yes in thermo - no in electro
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
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

16. Colligative properties
Same element - different number of neutrons
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
NH4?
Properties of solutions that depend on the number of particles per solvent molecule

17. Sterling silver
Mixture of silver and copper
Two compound react to form two new compounds
Decreased
Mixture of tin - copper - bismuth - and antimony

18. Solute vs. Solvent
The solute is dissolved in the solvent.
It is at equilibrium
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

19. Double replacement reaction
A compound breaks into two parts
Insoluble
Periods 8 and 9 - lanthanides and actinides
Two compound react to form two new compounds

20. Noble gas properties
4 bonding - 109.5° - sp³ hybridization
6 bonding - 90° - sp³d2² hybridization
Orange
Most stable

21. Ethanol
Stronger
Heat required to make a substance melt.
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

22. Color of excited Ba2+
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Light green
Most stable
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

23. Suspension
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
Strong acids - strong bases - soluble salts
Two reactants combine to form a single product

24. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
1st group - most reactive metal family - react violently with water - create basic solutions
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

25. Anhydride
CO - produced from incomplete combustion - very toxic
OH - alcohols - name ends in ol
Oxide that reacts with water to form either an acid or a base
Same formula - different structure

26. Charles' Law
Q = mcDT
Orange
V1/T1 = V2/T2
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

27. What qualifies as a strong base?
Acid to water
21% of atmosphere - colorless - odorless - supports combustion reactions
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Disordered systems with higher entropies are favored

28. Isomer
4.5 to 8.3 - Red to blue
Etching glass and frosting lightblubs
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Same formula - different structure

29. Molecular solids
C2H3O2?
Etching glass and frosting lightblubs
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

30. Metallic bonds
3 bonding - 1 nonbonding 107°
Electrons are free to move through metal structure - high conductivity - ductile
Mixture of silver and copper
Miscible with water - flammable - used as fuel - poisonous

31. What are the allotropic forms of sulfur?
Soluble
Gas pressure = atm pressure - height of mercury
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
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.

32. Alpha particle
Miscible with water - flammable - used as fuel - poisonous
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
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Same molecule - different electron pair positions

33. Positron emission
Soluble
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
It is at equilibrium
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

34. Phenolphthalein: pH range and colors
2 bonding - 1 nonbonding
Yes in thermo - no in electro
V1/T1 = V2/T2
8.3 to 10.0 - colorless to pink

35. Ketone
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Yes

36. Combustion reaction
3 bonding - 1 nonbonding 107°
Potassium - Calcium - Sodium
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
4 bonding - 109.5° - sp³ hybridization

37. Properties of ionic substances

38. Ammonium Ion
Orange
NH4?
Light green
Limited oxygen

39. Trigonal bipyramidal
Mixture of iron and carbon
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Gas pressure = atm pressure + height of mercury
5 bonding - 90° and 120° - sp³d hybridization

40. Silver bromide and silver iodide are used for
Photography
1st group - most reactive metal family - react violently with water - create basic solutions
Two compound react to form two new compounds
CO - produced from incomplete combustion - very toxic

41. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Yes in thermo - no in electro
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Soluble except when containing alkaline earth metals
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

42. Supersaturated solution
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
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
Orange
2 bonding - 180° - sp hybridization

43. Color of CrO4²? solution
Soluble except when containing alkaline earth metals
Q = mcDT
The solute is dissolved in the solvent.
Yellow

44. Azimuthal quantum number (l)
Defines shape of orbital
Glass and plastic
It is at equilibrium
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

45. Color of excited Fe3+
Gold
COH functional group - name ends in -al
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Light green

46. Dipole-dipole forces (including hydrogen bonds)
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Yes in thermo - no in electro

47. Linear
2 bonding - 180° - sp hybridization
1st group - most reactive metal family - react violently with water - create basic solutions
Etching glass and frosting lightblubs
4.184

48. Boyle's Law
M1V1 = M2V2
Stronger
P1/V1 = P2/V2
NH2 functional group - name ends in -amide

49. Covalent bond
Same molecule - different electron pair positions
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.
6 bonding - 90° - sp³d2² hybridization
COOH functional group - name ends in oic acid

50. Sulfide color: ZnS
Involves water
Magnesium
DG = DH - TDS
White