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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. Linear
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Disordered systems with higher entropies are favored
Excess oxygen
2 bonding - 180° - sp hybridization

2. Radioactivity
V1/T1 = V2/T2
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Blue-green

3. Solute vs. Solvent
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Disordered systems with higher entropies are favored
The solute is dissolved in the solvent.
Purple/pink

4. Compounds with 1-4 carbons
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Gases at room temperature - used for fuel
Diamond - graphite - amorphous - fullerenes
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

5. Color of excited K+
Involves water
SO4²?
The solute is dissolved in the solvent.
Purple/pink

6. Name the six strong acids
White
Extremely slow reactivity
Purple/pink
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

7. General Properties of Organic Compounds
Etching glass and frosting lightblubs
21% of atmosphere - colorless - odorless - supports combustion reactions
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Spin is +1/2 or -1/2 in an orbital

8. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Green
Liquid at room temperature - used to make gasoline and solvents
Yes in thermo - no in electro
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

9. London dispersion forces
21% of atmosphere - colorless - odorless - supports combustion reactions
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

10. Sigma bonds
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
NH4?
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Soluble

11. Halogens
Increased
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
7th group - form salts - always exist as diatomic molecules - used in modern lighting
NO3?

12. Cl - Br - and I compounds are...
Soluble except when containing Ag? - Hg2²? - or Pb²?
Black
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Miscible with water - flammable - used as fuel - poisonous

13. If G is negative - is the reaction spontaneous?
PO4³?
Classified as strong bases but not very soluble.
Yes
M1V1 = M2V2

14. Fission
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Energy level - as it increases electrons are less bound to the nucleus
Periods 8 and 9 - lanthanides and actinides
Orange

15. Chlorine gas
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Deadly - yellow-green - weapon
3 bonding - 1 nonbonding 107°
Solid at room temperature

16. Properties of molecular crystals and liquids

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17. Nitrate ion
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
NO3?
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
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

18. Ionic bond
Defines shape of orbital
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Substance can act either as an acid or a base
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

19. Resonance structures
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
Same molecule - different electron pair positions
C2H3O2?
Soluble

20. Acids with more oxygen atoms are
Excess oxygen
4.5 to 8.3 - Red to blue
Stronger
Glass and plastic

21. Phosphate ion
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
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
PO4³?
Two atoms with the same number of electrons

22. List equivalent pressure values for mmHg - torr - atm - and Pa
Glass and plastic
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Soluble
Orientation of orbital in space

23. Color of Ni2+ solution
Yes
Green
Extremely slow reactivity
Gold

24. amphoteric
Soluble
A compound breaks into two parts
Substance can act either as an acid or a base
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

25. Exceptions to the octet rule
Red
Etching glass and frosting lightblubs
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

26. Allotropic forms of carbon
NO3?
Diamond - graphite - amorphous - fullerenes
It is at equilibrium
Gold

27. Hydrofluoric acid is used for
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Red
Etching glass and frosting lightblubs
ClO3?

28. Trigonal bipyramidal
5 bonding - 90° and 120° - sp³d hybridization
Strong acids - strong bases - soluble salts
Most stable
Do not conduct electricity well

29. Sterling silver
Two compound react to form two new compounds
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
NH4?
Mixture of silver and copper

30. Pauli exclusion principle
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
DH = bonds broken - bonds formed
No two electrons can have the same set of 4 quantum numbers
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

31. Color of excited Na+
Two atoms with the same number of electrons
yellow
NH4?
Gas pressure = atm pressure + height of mercury

32. Covalent bond
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.
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Solid at room temperature
3.1 - 4.4 - red to yellow

33. Isotope
4.184
Same element - different number of neutrons
Energy level - as it increases electrons are less bound to the nucleus
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

34. Colligative properties
Excess oxygen
Two atoms with the same number of electrons
No
Properties of solutions that depend on the number of particles per solvent molecule

35. Amine group
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Orange
NH2 - ends in -amide
Miscible with water - flammable - used as fuel - poisonous

36. Ketone
Two atoms with the same number of electrons
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Two compound react to form two new compounds
Blue-green

37. If G is positive - is the reaction spontaneous?
No
Potassium - Calcium - Sodium
Disordered systems with higher entropies are favored
Yes

38. Fusion
Involves water
Most stable
2 bonding - 1 nonbonding
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

39. Electronegativity
Q = mcDT
Increase right and up
3 bonding - 1 nonbonding 107°
Acid to water

40. Add acid to water or water to acid
Acid to water
4 bonding - 109.5° - sp³ hybridization
3 bonding - 1 nonbonding 107°
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

41. Acetate ion
7th group - form salts - always exist as diatomic molecules - used in modern lighting
More active element replaces less active element in a compound.
4.184
C2H3O2?

42. Brass
Mixture of copper and zinc
Glass and plastic
R-O-R functional group - shorter chain ends in oxy - other is ane
Increase right and up

43. Alkali metal compounds and NH4? compounds are...
21% of atmosphere - colorless - odorless - supports combustion reactions
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Soluble
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

44. Color of Cu2+ solution
Yes in thermo - no in electro
Make up jet fuels and kerosene
Same formula - different structure
Blue

45. Carboxylic acid
COOH functional group - name ends in oic acid
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
Stronger
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

46. What are the factors that affect reaction rate?
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Two atoms with the same number of electrons
More active element replaces less active element in a compound.
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

47. Steel
Solid at room temperature
Mixture of iron and carbon
2 bonding - 180° - sp hybridization
4.184

48. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Emission of electromagnetic energy after beta - positron - or alpha decay

49. Examples of strong electrolytes
Strong acids - strong bases - soluble salts
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Yellow

50. Pi bonds
Decreased
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Increased
Properties of solutions that depend on the number of particles per solvent molecule