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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. Alkaline metal oxides are...
NH2 functional group - name ends in -amide
Classified as strong bases but not very soluble.
It is at equilibrium
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

2. Aldehydes
COH functional group - name ends in -al
Involves water
Stronger
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

3. Colligative properties
Same formula - different structure
Etching glass and frosting lightblubs
Spin is +1/2 or -1/2 in an orbital
Properties of solutions that depend on the number of particles per solvent molecule

4. Solute vs. Solvent
Orange
The solute is dissolved in the solvent.
Etching glass and frosting lightblubs
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

5. Cl - Br - and I compounds are...
Potassium - Calcium - Sodium
Soluble except when containing Ag? - Hg2²? - or Pb²?
Yellow
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

6. Acetate ion
Increased
C2H3O2?
Strong acids - strong bases - soluble salts
Emission of electromagnetic energy after beta - positron - or alpha decay

7. Name the six strong acids
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Mixture of copper - zinc - and other metals
7th group - form salts - always exist as diatomic molecules - used in modern lighting
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

8. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Degrade the oxone layer
COOH - ends in -oic acid
Yes in thermo - no in electro
DG = DH - TDS

9. Octahedral
Covalent
6 bonding - 90° - sp³d2² hybridization
Same formula - different structure
Low pressures - high temperatures

10. Carbonate ion
CO3²?
Decreased
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
DH = bonds broken - bonds formed

11. Radioactivity
Increased
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
P1/V1 = P2/V2
21% of atmosphere - colorless - odorless - supports combustion reactions

12. Coal
Make up jet fuels and kerosene
Strong acids - strong bases - soluble salts
PV = nRT - R = .0821
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

13. Graham's Law
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Substance can act either as an acid or a base
1st group - most reactive metal family - react violently with water - create basic solutions

14. Alkali Metals
1st group - most reactive metal family - react violently with water - create basic solutions
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
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)

15. Compounds with 12-18 carbons
R-O-R functional group - shorter chain ends in oxy - other is ane
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Two reactants combine to form a single product
Make up jet fuels and kerosene

16. pewter
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
M1V1 = M2V2
Diamond - graphite - amorphous - fullerenes
Mixture of tin - copper - bismuth - and antimony

17. Is removing an electron an exothermic or endothermic process?
yellow
Properties of solutions that depend on the number of particles per solvent molecule
Endothermic
Soluble

18. Color of Cu2+ solution
PO4³?
Blue
Yellow
Glass and plastic

19. List equivalent pressure values for mmHg - torr - atm - and Pa
Nonmetal oxides form acids - metal oxides form bases
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

20. bronze
Mixture of copper - zinc - and other metals
Potassium - Calcium - Sodium
5 bonding - 90° and 120° - sp³d hybridization
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

21. Pi bonds
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
2nd group - fairly reactive - pastes are used in batteries
Oxide that reacts with water to form either an acid or a base
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

22. Noble gas properties
Most stable
Soluble
Excess oxygen
Moles / L

23. Compounds with 18 carbons
Solid at room temperature
COOH functional group - name ends in oic acid
CO3²?
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

24. Allotropic forms of carbon
Gases at room temperature - used for fuel
Diamond - graphite - amorphous - fullerenes
No two electrons can have the same set of 4 quantum numbers
yellow

25. Hydrogen gas properties
1st group - most reactive metal family - react violently with water - create basic solutions
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
5 bonding - 90° and 120° - sp³d hybridization
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

26. Complete combustion occurs when there is
Degrade the oxone layer
5 bonding - 90° and 120° - sp³d hybridization
Excess oxygen
Q = mcDT

27. Gibb's Free Energy equation
DG = DH - TDS
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
No
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

28. Color of Ni2+ solution
Periods 8 and 9 - lanthanides and actinides
Defines shape of orbital
Green
OH - alcohols - name ends in ol

29. Color of excited K+
Purple/pink
OH functional group - name ends in -ol
PO4³?
Strong acids - strong bases - soluble salts

30. Dipole-dipole forces (including hydrogen bonds)
21% of atmosphere - colorless - odorless - supports combustion reactions
3.1 - 4.4 - red to yellow
Yes in thermo - no in electro
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

31. Color of excited Ba2+
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
Light 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

32. Trigonal bipyramidal
5 bonding - 90° and 120° - sp³d hybridization
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
COOH - ends in -oic acid
Purple

33. Add acid to water or water to acid
6.0 to 7.6 - yellow to blue
Acid to water
M1V1 = M2V2
6 bonding - 90° - sp³d2² hybridization

34. Carbon dioxide gas properties
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
C2H3O2?
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

35. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Soluble
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Yellow to orange
2 bonding - 180° - sp hybridization

36. Color of excited Li+ - Sr2+ - Ca2+
Magnesium
Miscible with water - flammable - used as fuel - poisonous
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Red

37. Noble gases
Extremely slow reactivity
Limited oxygen
Two atoms with the same number of electrons
Red

38. F compounds are...
Photography
Soluble except when containing alkaline earth metals
Same formula - different structure
6 bonding - 90° - sp³d2² hybridization

39. Properties of ionic substances

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40. Phosphate ion
PO4³?
P1/V1 = P2/V2
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
4 bonding - 109.5° - sp³ hybridization

41. Methanol
Miscible with water - flammable - used as fuel - poisonous
Electrons are free to move through metal structure - high conductivity - ductile
Periods 8 and 9 - lanthanides and actinides
8.3 to 10.0 - colorless to pink

42. What is the ideal gas law?
Two compound react to form two new compounds
PV = nRT - R = .0821
C2H3O2?
2 bonding - 180° - sp hybridization

43. Molarity
Moles / L
Glass and plastic
Insoluble
Spin is +1/2 or -1/2 in an orbital

44. If G is negative - is the reaction spontaneous?
Soluble except when containing alkaline earth metals
Covalent
Disordered systems with higher entropies are favored
Yes

45. Alkali metal properties
Spin is +1/2 or -1/2 in an orbital
6.0 to 7.6 - yellow to blue
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
NH2 - ends in -amide

46. Isomer
Strong acids - strong bases - soluble salts
Light green
Increases left and down
Same formula - different structure

47. What kind of bonds generally hold gases together?
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
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
Light green
Covalent

48. Acids with more oxygen atoms are
OH functional group - name ends in -ol
8.3 to 10.0 - colorless to pink
Purple/pink
Stronger

49. Silver bromide and silver iodide are used for
Nonmetal oxides form acids - metal oxides form bases
DG = DH - TDS
Photography
Yellow

50. Chlorofluorocarbons
Degrade the oxone layer
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
C2H3O2?
Emission of electromagnetic energy after beta - positron - or alpha decay