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SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Aldehydes
COH functional group - name ends in -al
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Defines shape of orbital
ClO3?

2. How many joules are in a calorie?
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Deadly - yellow-green - weapon
A compound breaks into two parts
4.184

3. Fusion
Same molecule - different electron pair positions
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Yellow
Extremely slow reactivity

4. Compounds with 5-10 carbons
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Miscible with water - flammable - used as fuel - poisonous
Same formula - different structure
Liquid at room temperature - used to make gasoline and solvents

5. Trigonal planar
CO3²?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
3 bonding - 120° - sp² hybridization

6. Carbon monoxide
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
CO - produced from incomplete combustion - very toxic
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
8.3 to 10.0 - colorless to pink

7. London dispersion forces
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Two atoms with the same number of electrons

8. Exceptions to the octet rule
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Mixture of iron and carbon
Bright yellow
P1/V1 = P2/V2

9. Sulfide color: As2S3
Lemon yellow
COOH - ends in -oic acid
Black
Orientation of orbital in space

10. Methyl orange: pH range and colors
yellow
OH functional group - name ends in -ol
3.1 - 4.4 - red to yellow
A compound breaks into two parts

11. Radioactivity
Orange
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Increases left and down
Gas pressure = atm pressure - height of mercury

12. Covalent-network / atomic solids
Orange
Limited oxygen
NH2 - ends in -amide
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

13. Supersaturated solution
Spin is +1/2 or -1/2 in an orbital
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Involves water
Oxide that reacts with water to form either an acid or a base

14. Color of MnO4? solution
Low pressures - high temperatures
Same formula - different structure
Purple
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

15. Boyle's Law
Same formula - different structure
No two electrons can have the same set of 4 quantum numbers
P1/V1 = P2/V2
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

16. Acetate ion
C2H3O2?
5 bonding - 90° and 120° - sp³d hybridization
P1/V1 = P2/V2
PO4³?

17. Examples of strong electrolytes
Oxide that reacts with water to form either an acid or a base
Q = mcDT
Strong acids - strong bases - soluble salts
Red

18. Sulfate ion
SO4²?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
COOH functional group - name ends in oic acid

19. Petroleum
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Blue
Red

20. Add acid to water or water to acid
Q = mcDT
Acid to water
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
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.

21. Sulfide color: ZnS
Lemon yellow
Bright yellow
Energy level - as it increases electrons are less bound to the nucleus
White

22. Azimuthal quantum number (l)
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Purple/pink
Defines shape of orbital
Diamond - graphite - amorphous - fullerenes

23. Silver bromide and silver iodide are used for
Green
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
Photography
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

24. pewter
V1/T1 = V2/T2
Mixture of tin - copper - bismuth - and antimony
Orange
Magnesium

25. Linear
More active element replaces less active element in a compound.
Two compound react to form two new compounds
Miscible with water - flammable - used as fuel - poisonous
2 bonding - 180° - sp hybridization

26. Principal quantum number (n)
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Yellow to orange
Energy level - as it increases electrons are less bound to the nucleus
Moles of solute / kg solvent

27. bronze
Classified as strong bases but not very soluble.
Green
Mixture of copper - zinc - and other metals
Covalent

28. SO4²? compounds are...
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
NO3?

29. Carboxylic acid
COOH functional group - name ends in oic acid
7th group - form salts - always exist as diatomic molecules - used in modern lighting
COH functional group - name ends in -al
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

30. Dilution equation
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
Yellow
Soluble except when containing Ag? - Hg2²? - or Pb²?
M1V1 = M2V2

31. Ionic bond
Extremely slow reactivity
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Moles of solute / kg solvent
Magnesium

32. Metallic solids
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Orientation of orbital in space
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
8.3 to 10.0 - colorless to pink

33. Steel
Endothermic
Decreased
Mixture of iron and carbon
Light green

34. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Miscible with water - flammable - used as fuel - poisonous
COOH functional group - name ends in oic acid
ClO3?

35. Magnetic quantum number (ml)
NO3?
Orientation of orbital in space
Diamond - graphite - amorphous - fullerenes
Moles of solute / kg solvent

36. Phenolphthalein: pH range and colors
8.3 to 10.0 - colorless to pink
Gold
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Extremely slow reactivity

37. Hydrogen gas properties
Nonmetal oxides form acids - metal oxides form bases
Disordered systems with higher entropies are favored
21% of atmosphere - colorless - odorless - supports combustion reactions
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

38. Equation when using a barometer to calculate gas pressure.
White
NH2 - ends in -amide
Gas pressure = atm pressure - height of mercury
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

39. Resonance structures
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
Same molecule - different electron pair positions
2 bonding - 180° - sp hybridization
Same element - different number of neutrons

40. Properties of ionic substances

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41. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Acid to water
Yes in thermo - no in electro
Lemon yellow
Disordered systems with higher entropies are favored

42. Noble gas properties
Mixture of silver and copper
NO3?
Most stable
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

43. Properties of molecular crystals and liquids

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44. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
2 bonding - 180° - sp hybridization
Diamond - graphite - amorphous - fullerenes
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

45. Pauli exclusion principle
Gold
No two electrons can have the same set of 4 quantum numbers
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

46. Ammonium Ion
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
NH4?
OH - alcohols - name ends in ol
Electrons are free to move through metal structure - high conductivity - ductile

47. Pi bonds
Defines shape of orbital
Covalent
No two electrons can have the same set of 4 quantum numbers
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

48. Sulfide color: CuS - HgS - and PbS
Black
R-O-R functional group - shorter chain ends in oxy - other is ane
Mixture of copper - zinc - and other metals
Light green

49. Chlorate ion
ClO3?
Orientation of orbital in space
Disordered systems with higher entropies are favored
Excess oxygen

50. Properties of bases
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
COH functional group - name ends in -al
Mixture of silver and copper
Orange