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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. Litmus: pH range and colors
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
4.5 to 8.3 - Red to blue
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Mixture of iron and carbon

2. Carbon monoxide
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Covalent
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
CO - produced from incomplete combustion - very toxic

3. Electron affinity
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Nonmetal oxides form acids - metal oxides form bases
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
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

4. Molality
DG = DH - TDS
Moles of solute / kg solvent
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
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

5. Spin quantum number (ms)
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Spin is +1/2 or -1/2 in an orbital
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Blue-green

6. Halogens
Gas pressure = atm pressure - height of mercury
DG = DH - TDS
NH2 - ends in -amide
7th group - form salts - always exist as diatomic molecules - used in modern lighting

7. Ionic solids
Mixture of tin - copper - bismuth - and antimony
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Two reactants combine to form a single product
NH4?

8. Bent
Classified as strong bases but not very soluble.
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Q = mcDT
2 bonding - 1 nonbonding

9. Color of excited Na+
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Same formula - different structure
Mixture of copper - zinc - and other metals
yellow

10. What qualifies as a strong base?
Gas pressure = atm pressure + height of mercury
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
CO - produced from incomplete combustion - very toxic
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

11. Magnetic quantum number (ml)
Moles of solute / kg solvent
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
NH4?
Orientation of orbital in space

12. Boiling point elevation formula
Classified as strong bases but not very soluble.
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Nonmetal oxides form acids - metal oxides form bases
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

13. Ionic bond
Mixture of copper - zinc - and other metals
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Orange
Orientation of orbital in space

14. Metallic bonds
3 bonding - 120° - sp² hybridization
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Electrons are free to move through metal structure - high conductivity - ductile
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

15. Radioactivity
Moles of solute / kg solvent
Potassium - Calcium - Sodium
ClO3?
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

16. pewter
Yellow
Mixture of tin - copper - bismuth - and antimony
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Soluble

17. Cl - Br - and I compounds are...
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Soluble except when containing Ag? - Hg2²? - or Pb²?
Properties of solutions that depend on the number of particles per solvent molecule

18. Gibb's Free Energy equation
Same element - different number of neutrons
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Light green
DG = DH - TDS

19. Trigonal bipyramidal
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Classified as strong bases but not very soluble.
5 bonding - 90° and 120° - sp³d hybridization
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

20. Ionization energy
Heat required to make a substance melt.
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

21. How can hydrogen be produced?
Green
Decreased
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Periods 8 and 9 - lanthanides and actinides

22. Isomer
Same formula - different structure
Blue
V1/T1 = V2/T2
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

23. Transition metals
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Gold
Magnesium
Oxide that reacts with water to form either an acid or a base

24. How many joules are in a calorie?
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
4.184
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
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

25. amphoteric
Yellow to orange
Substance can act either as an acid or a base
8.3 to 10.0 - colorless to pink
Extremely slow reactivity

26. Compounds with 5-10 carbons
Pressure of mixture of gases equals some of individual gas pressures.
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Liquid at room temperature - used to make gasoline and solvents
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

27. Alkaline earth metals
Gold
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
M1V1 = M2V2
2nd group - fairly reactive - pastes are used in batteries

28. What are the allotropic forms of sulfur?
Yes
SO4²?
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

29. Properties of acids
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Deadly - yellow-green - weapon
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

30. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Classified as strong bases but not very soluble.
Two compound react to form two new compounds
PO4³?
Insoluble

31. Ethanol
Bright yellow
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Light green
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

32. Petroleum
COOH functional group - name ends in oic acid
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Properties of solutions that depend on the number of particles per solvent molecule
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

33. Covalent-network / atomic solids
Covalent
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Miscible with water - flammable - used as fuel - poisonous

34. Freezing point depression formula
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
No two electrons can have the same set of 4 quantum numbers
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Yes in thermo - no in electro

35. Alkaline metal oxides are...
Soluble
It is at equilibrium
Potassium - Calcium - Sodium
Classified as strong bases but not very soluble.

36. Sulfide color: CdS
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Bright yellow
More active element replaces less active element in a compound.
Increases left and down

37. Color of Cu2+ solution
Decreased
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Blue
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

38. Graham's Law
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
3 bonding - 120° - sp² hybridization

39. What metal will react in hot water?
Soluble
Mixture of copper and zinc
Magnesium
Bright yellow

40. Chlorate ion
Emission of electromagnetic energy after beta - positron - or alpha decay
ClO3?
Two reactants combine to form a single product
Decreased

41. Compounds with 18 carbons
Solid at room temperature
It is at equilibrium
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Soluble

42. Hydroxyl group
OH - alcohols - name ends in ol
Mixture of tin - copper - bismuth - and antimony
M1V1 = M2V2
Limited oxygen

43. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Yes in thermo - no in electro
yellow
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Etching glass and frosting lightblubs

44. Solute vs. Solvent
NH2 functional group - name ends in -amide
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
It is at equilibrium
The solute is dissolved in the solvent.

45. Noble gas properties
Most stable
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
8.3 to 10.0 - colorless to pink
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

46. Molarity
Moles of solute / kg solvent
3.1 - 4.4 - red to yellow
Moles / L
Mixture of copper - zinc - and other metals

47. Sterling silver
Covalent
4.5 to 8.3 - Red to blue
Mixture of silver and copper
Same molecule - different electron pair positions

48. Incomplete combustion occurs when there is
Classified as strong bases but not very soluble.
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
White
Limited oxygen

49. Color of CrO4²? solution
Photography
Yellow
Light green
C2H3O2?

50. Hydrogen gas properties
Periods 8 and 9 - lanthanides and actinides
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Photography
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond