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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. Bromthymol blue: pH range and colors
Heat required to make a substance melt.
Strong acids - strong bases - soluble salts
6.0 to 7.6 - yellow to blue
1st group - most reactive metal family - react violently with water - create basic solutions

2. Bent
PV = nRT - R = .0821
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
2 bonding - 1 nonbonding
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

3. Acids with more oxygen atoms are
Stronger
Excess oxygen
It is at equilibrium
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

4. Carbon monoxide
Properties of solutions that depend on the number of particles per solvent molecule
CO - produced from incomplete combustion - very toxic
Gas pressure = atm pressure - height of mercury
Stronger

5. Supersaturated solution
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
COOH functional group - name ends in oic acid
Soluble except when containing alkaline earth metals

6. Ester
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
M1V1 = M2V2
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

7. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
2 bonding - 180° - sp hybridization
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

8. Color of Fe3+ solution
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
PV = nRT - R = .0821
Yellow to orange
Soluble except when containing alkaline earth metals

9. Suspension
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
The solute is dissolved in the solvent.
Blue
4 bonding - 109.5° - sp³ hybridization

10. General properties of alloys
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
More active element replaces less active element in a compound.
Photography
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

11. Hydroxyl group
4.184
OH - alcohols - name ends in ol
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

12. Oxygen gas properties
CO - produced from incomplete combustion - very toxic
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Liquid at room temperature - used to make gasoline and solvents
21% of atmosphere - colorless - odorless - supports combustion reactions

13. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
Make up jet fuels and kerosene
It is at equilibrium
M1V1 = M2V2

14. Compounds with 1-4 carbons
Mixture of tin - copper - bismuth - and antimony
Gases at room temperature - used for fuel
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Energy level - as it increases electrons are less bound to the nucleus

15. Positron emission
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Etching glass and frosting lightblubs
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

16. Carbon dioxide gas properties
Disordered systems with higher entropies are favored
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 iron and carbon
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

17. Hydrogen gas properties
OH - alcohols - name ends in ol
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Oxide that reacts with water to form either an acid or a base
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

18. Molecular solids
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Miscible with water - flammable - used as fuel - poisonous
Oxide that reacts with water to form either an acid or a base
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

19. Color of excited Ba2+
Low pressures - high temperatures
Light green
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Orange

20. Ionization energy
Soluble except when containing Ag? - Hg2²? - or Pb²?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
yellow
P1/V1 = P2/V2

21. Color of CrO7²? solution
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Yes
3 bonding - 120° - sp² hybridization
Orange

22. Alchohols
OH functional group - name ends in -ol
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Etching glass and frosting lightblubs

23. Add acid to water or water to acid
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Two atoms with the same number of electrons
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Acid to water

24. amphoteric
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Substance can act either as an acid or a base
Decreased
1st group - most reactive metal family - react violently with water - create basic solutions

25. Sulfide color: CuS - HgS - and PbS
Lemon yellow
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Black
NH2 functional group - name ends in -amide

26. If G is positive - is the reaction spontaneous?
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Pressure of mixture of gases equals some of individual gas pressures.
NH2 - ends in -amide
No

27. Color of excited Li+ - Sr2+ - Ca2+
Red
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
2 bonding - 180° - sp hybridization
Gases at room temperature - used for fuel

28. Decomposition reaction
Q = mcDT
A compound breaks into two parts
Acid to water
Yes in thermo - no in electro

29. Properties of ionic substances

30. Properties of acids
Orange
Increase right and up
Potassium - Calcium - Sodium
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

31. Incomplete combustion occurs when there is
Limited oxygen
Lemon yellow
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

32. Transition metals
Endothermic
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

33. Chlorine gas
Red
Deadly - yellow-green - weapon
Bright yellow
Gold

34. Compounds with 5-10 carbons
Orange
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Liquid at room temperature - used to make gasoline and solvents
Mixture of tin - copper - bismuth - and antimony

35. Phenolphthalein: pH range and colors
Defines shape of orbital
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
8.3 to 10.0 - colorless to pink
Light green

36. Molarity
R-O-R functional group - shorter chain ends in oxy - other is ane
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
4.184
Moles / L

37. Alkali metal compounds and NH4? compounds are...
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 to orange
Stronger
Soluble

38. Gibb's Free Energy equation
Increases left and down
DG = DH - TDS
Emission of electromagnetic energy after beta - positron - or alpha decay
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

39. List equivalent pressure values for mmHg - torr - atm - and Pa
Increased
Degrade the oxone layer
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Defines shape of orbital

40. Sulfide color: As2S3
Potassium - Calcium - Sodium
Decreased
Orientation of orbital in space
Lemon yellow

41. Color of excited K+
4.5 to 8.3 - Red to blue
PO4³?
Purple/pink
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

42. What metal will react in hot water?
3.1 - 4.4 - red to yellow
3 bonding - 120° - sp² hybridization
Magnesium
1st group - most reactive metal family - react violently with water - create basic solutions

43. Sulfide color: CdS
Heat required to make a substance melt.
Bright yellow
Yes in thermo - no in electro
Mixture of copper - zinc - and other metals

44. F compounds are...
C2H3O2?
White
Soluble except when containing alkaline earth metals
Photography

45. Carbonate ion
Increase right and up
4.5 to 8.3 - Red to blue
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
CO3²?

46. Resonance structures
P1/V1 = P2/V2
Nonmetal oxides form acids - metal oxides form bases
PV = nRT - R = .0821
Same molecule - different electron pair positions

47. Sigma bonds
Increase right and up
Increased
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Defines shape of orbital

48. Trigonal planar
DH = bonds broken - bonds formed
3 bonding - 120° - sp² hybridization
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
2nd group - fairly reactive - pastes are used in batteries

49. What kind of bonds generally hold gases together?
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
Covalent
Blue-green
Yes in thermo - no in electro

50. Amine
NH2 functional group - name ends in -amide
Blue-green
Increases left and down
Same formula - different structure

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SAT Subject Test: Chemistry

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