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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. Isomer
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Mixture of tin - copper - bismuth - and antimony
Same formula - different structure
Two compound react to form two new compounds

2. Nonmetals
Do not conduct electricity well
Heat required to make a substance melt.
21% of atmosphere - colorless - odorless - supports combustion reactions
Emission of electromagnetic energy after beta - positron - or alpha decay

3. Tetrahedral
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
Oxide that reacts with water to form either an acid or a base
4 bonding - 109.5° - sp³ hybridization
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

4. Color of excited Na+
Soluble except when containing Ag? - Hg2²? - or Pb²?
PO4³?
Spin is +1/2 or -1/2 in an orbital
yellow

5. Pauli exclusion principle
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
No two electrons can have the same set of 4 quantum numbers
Blue
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

6. Boyle's Law
Orange
P1/V1 = P2/V2
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Mixture of copper - zinc - and other metals

7. Examples of amorphous solids
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
Glass and plastic
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
Purple

8. What kind of bonds generally hold gases together?
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Decreased
Covalent
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

9. Is removing an electron an exothermic or endothermic process?
Spin is +1/2 or -1/2 in an orbital
6 bonding - 90° - sp³d2² hybridization
2nd group - fairly reactive - pastes are used in batteries
Endothermic

10. Pi bonds
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Degrade the oxone layer
ClO3?
COOH functional group - name ends in oic acid

11. Color of Fe3+ solution
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Increase right and up
Liquid at room temperature - used to make gasoline and solvents
Yellow to orange

12. Ionization energy
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Decreased
6 bonding - 90° - sp³d2² hybridization
Purple/pink

13. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Periods 8 and 9 - lanthanides and actinides
Degrade the oxone layer
Gas pressure = atm pressure + height of mercury

14. Carbon monoxide
CO - produced from incomplete combustion - very toxic
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Gas pressure = atm pressure - height of mercury
M1V1 = M2V2

15. Carbon dioxide gas properties
4.5 to 8.3 - Red to blue
Soluble
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
PV = nRT - R = .0821

16. Ester
Purple/pink
21% of atmosphere - colorless - odorless - supports combustion reactions
COOH - ends in -oic acid
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

17. Color of excited Cu2+
Blue-green
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Gas pressure = atm pressure + height of mercury
Bright yellow

18. Carboxylic acid
COOH functional group - name ends in oic acid
ClO3?
Gases at room temperature - used for fuel
8.3 to 10.0 - colorless to pink

19. Dipole-dipole forces (including hydrogen bonds)
Mixture of copper and zinc
White
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

20. When a reaction is endothermic - the entropy is
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Increased
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

21. Colloid
Stronger
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
8.3 to 10.0 - colorless to pink
Potassium - Calcium - Sodium

22. Hydrogen gas properties
Covalent
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
3 bonding - 120° - sp² hybridization
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

23. What 3 metals will react with cold water?
5 bonding - 90° and 120° - sp³d hybridization
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Potassium - Calcium - Sodium
Involves water

24. Molality
Extremely slow reactivity
SO4²?
Purple
Moles of solute / kg solvent

25. If G is negative - is the reaction spontaneous?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
White
Limited oxygen
Yes

26. Chlorate ion
ClO3?
COOH - ends in -oic acid
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Heat required to make a substance melt.

27. Rare earth elements
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Mixture of silver and copper
Potassium - Calcium - Sodium
Periods 8 and 9 - lanthanides and actinides

28. Noble gas properties
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Mixture of tin - copper - bismuth - and antimony
Most stable
Two reactants combine to form a single product

29. Compounds with 18 carbons
Increases left and down
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
Solid at room temperature
NH4?

30. Brass
Solid at room temperature
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
2 bonding - 180° - sp hybridization
Mixture of copper and zinc

31. Compounds with 1-4 carbons
Involves water
No
Gases at room temperature - used for fuel
Soluble

32. Color of CrO4²? solution
Most stable
Yellow
1st group - most reactive metal family - react violently with water - create basic solutions
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

33. Properties of molecular crystals and liquids

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34. Beta particle
Classified as strong bases but not very soluble.
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

35. Azimuthal quantum number (l)
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
5 bonding - 90° and 120° - sp³d hybridization
2nd group - fairly reactive - pastes are used in batteries
Defines shape of orbital

36. Freezing point depression formula
V1/T1 = V2/T2
Gas pressure = atm pressure - height of mercury
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

37. Halogen properties
Classified as strong bases but not very soluble.
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Strong acids - strong bases - soluble salts
M1V1 = M2V2

38. Silver bromide and silver iodide are used for
COH functional group - name ends in -al
Photography
Most stable
Covalent

39. Add acid to water or water to acid
Acid to water
COH functional group - name ends in -al
R-O-R functional group - shorter chain ends in oxy - other is ane
ClO3?

40. Steel
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Liquid at room temperature - used to make gasoline and solvents
Mixture of iron and carbon
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

41. pewter
Stronger
Mixture of tin - copper - bismuth - and antimony
Covalent
yellow

42. Graham's Law
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
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.
4.184

43. Octahedral
No two electrons can have the same set of 4 quantum numbers
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
6 bonding - 90° - sp³d2² hybridization
V1/T1 = V2/T2

44. Alkaline metal oxides are...
Classified as strong bases but not very soluble.
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Bright yellow
Glass and plastic

45. Color of Ni2+ solution
Yellow to orange
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Green
Mixture of copper and zinc

46. Isotope
2 bonding - 180° - sp hybridization
Mixture of tin - copper - bismuth - and antimony
Emission of electromagnetic energy after beta - positron - or alpha decay
Same element - different number of neutrons

47. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Miscible with water - flammable - used as fuel - poisonous
Insoluble
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

48. Compounds with 12-18 carbons
Make up jet fuels and kerosene
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
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
Soluble

49. Properties of ionic substances

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50. Alkali metal properties
Properties of solutions that depend on the number of particles per solvent molecule
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Heat required to make a substance melt.
COH functional group - name ends in -al