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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. Coal
Defines shape of orbital
6.0 to 7.6 - yellow to blue
Mixture of copper and zinc
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

2. Name the six strong acids
Mixture of copper - zinc - and other metals
Magnesium
Q = mcDT
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

3. Octahedral
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
6 bonding - 90° - sp³d2² hybridization
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

4. What kind of bonds generally hold liquids together?
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
2 bonding - 180° - sp hybridization
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Covalent

5. When the reaction is exothermic - the entropy is
Most stable
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
C2H3O2?
Decreased

6. SO4²? compounds are...
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Pressure of mixture of gases equals some of individual gas pressures.
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
No two electrons can have the same set of 4 quantum numbers

7. Transition metals
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
2 bonding - 1 nonbonding
Degrade the oxone layer

8. Equation when using a barometer to calculate gas pressure.
SO4²?
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Increased
Gas pressure = atm pressure - height of mercury

9. Azimuthal quantum number (l)
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
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
No
Defines shape of orbital

10. Sulfide color: CuS - HgS - and PbS
Etching glass and frosting lightblubs
Black
2 bonding - 1 nonbonding
Moles of solute / kg solvent

11. Properties of ionic substances

12. Covalent-network / atomic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Same element - different number of neutrons
Stronger

13. Ionization energy
NH2 - ends in -amide
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

14. General Properties of Organic Compounds
DG = DH - TDS
Energy level - as it increases electrons are less bound to the nucleus
Same element - different number of neutrons
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

15. Bromthymol blue: pH range and colors
Acid to water
6.0 to 7.6 - yellow to blue
Nonmetal oxides form acids - metal oxides form bases
Low pressures - high temperatures

16. Single Replacement / displacement reaction
Gas pressure = atm pressure - height of mercury
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
More active element replaces less active element in a compound.

17. Molality
8.3 to 10.0 - colorless to pink
2 bonding - 180° - sp hybridization
Moles of solute / kg solvent
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

18. Isotope
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Same element - different number of neutrons
It is at equilibrium
Increases left and down

19. Steel
Oxide that reacts with water to form either an acid or a base
Mixture of iron and carbon
Degrade the oxone layer
2 bonding - 180° - sp hybridization

20. Pauli exclusion principle
3 bonding - 1 nonbonding 107°
No two electrons can have the same set of 4 quantum numbers
Electrons are free to move through metal structure - high conductivity - ductile
Substance can act either as an acid or a base

21. Rare earth elements
2nd group - fairly reactive - pastes are used in batteries
White
ClO3?
Periods 8 and 9 - lanthanides and actinides

22. Alkali metal compounds and NH4? compounds are...
ClO3?
2nd group - fairly reactive - pastes are used in batteries
More active element replaces less active element in a compound.
Soluble

23. Boyle's Law
P1/V1 = P2/V2
Purple
Lemon yellow
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

24. Boiling point elevation formula
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
CO - produced from incomplete combustion - very toxic
Degrade the oxone layer
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

25. Chlorate ion
Photography
2 bonding - 1 nonbonding
ClO3?
Blue-green

26. Sulfide color: As2S3
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
Lemon yellow
Soluble
Photography

27. Is removing an electron an exothermic or endothermic process?
Pressure of mixture of gases equals some of individual gas pressures.
Disordered systems with higher entropies are favored
Endothermic
Mixture of copper and zinc

28. Phenolphthalein: pH range and colors
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
8.3 to 10.0 - colorless to pink
NH4?
Moles / L

29. Noble gases
Extremely slow reactivity
1st group - most reactive metal family - react violently with water - create basic solutions
Two reactants combine to form a single product
Periods 8 and 9 - lanthanides and actinides

30. Noble gas properties
Most stable
Involves water
OH functional group - name ends in -ol
4.5 to 8.3 - Red to blue

31. Atomic radius trend
Acid to water
Increases left and down
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

32. Formula for calculating enthalpy change with bond energies
No two electrons can have the same set of 4 quantum numbers
DH = bonds broken - bonds formed
Properties of solutions that depend on the number of particles per solvent molecule
Covalent

33. What metal will react in hot water?
6.0 to 7.6 - yellow to blue
2 bonding - 180° - sp hybridization
Purple/pink
Magnesium

34. Combustion reaction
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Blue
3 bonding - 1 nonbonding 107°
Involves water

35. Alchohols
M1V1 = M2V2
Orientation of orbital in space
OH functional group - name ends in -ol
Potassium - Calcium - Sodium

36. Bent
Same molecule - different electron pair positions
2 bonding - 1 nonbonding
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Mixture of silver and copper

37. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
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
Mixture of copper - zinc - and other metals
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Yes in thermo - no in electro

38. What kind of bonds generally hold gases together?
Emission of electromagnetic energy after beta - positron - or alpha decay
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Covalent
Energy level - as it increases electrons are less bound to the nucleus

39. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
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.
Increased
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

40. Beta particle
Moles / L
4.5 to 8.3 - Red to blue
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

41. Silver bromide and silver iodide are used for
Photography
White
Involves water
SO4²?

42. If G is negative - is the reaction spontaneous?
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
4.5 to 8.3 - Red to blue
Yes
Red

43. Radioactivity
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

44. What is the second law of thermodynamics?
Two reactants combine to form a single product
Yellow to orange
Disordered systems with higher entropies are favored
ClO3?

45. Principal quantum number (n)
COH functional group - name ends in -al
Blue-green
Energy level - as it increases electrons are less bound to the nucleus
Extremely slow reactivity

46. Sigma bonds
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
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
3.1 - 4.4 - red to yellow
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

47. Ethers
Mixture of silver and copper
5 bonding - 90° and 120° - sp³d hybridization
R-O-R functional group - shorter chain ends in oxy - other is ane
Same molecule - different electron pair positions

48. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Defines shape of orbital
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
Gas pressure = atm pressure + height of mercury
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

49. Graham's Law
COOH - ends in -oic acid
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Purple
6.0 to 7.6 - yellow to blue

50. Methanol
Electrons are free to move through metal structure - high conductivity - ductile
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Miscible with water - flammable - used as fuel - poisonous
yellow