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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. Ethers
COOH - ends in -oic acid
R-O-R functional group - shorter chain ends in oxy - other is ane
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

2. Nitrate ion
Lemon yellow
Gas pressure = atm pressure + height of mercury
NO3?
Soluble except when containing Ag? - Hg2²? - or Pb²?

3. Alkaline earth metals
Soluble
Magnesium
2nd group - fairly reactive - pastes are used in batteries
Defines shape of orbital

4. Freezing point depression formula
Increased
Energy level - as it increases electrons are less bound to the nucleus
Magnesium
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

5. Sulfide color: As2S3
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Soluble
Lemon yellow
Moles of solute / kg solvent

6. Carbon dioxide gas properties
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
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Mixture of iron and carbon

7. Examples of strong electrolytes
Strong acids - strong bases - soluble salts
CO - produced from incomplete combustion - very toxic
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

8. Azimuthal quantum number (l)
Defines shape of orbital
No two electrons can have the same set of 4 quantum numbers
CO3²?
Electrons are free to move through metal structure - high conductivity - ductile

9. Noble gases
M1V1 = M2V2
Extremely slow reactivity
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

10. Metallic solids
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Gold
2 bonding - 180° - sp hybridization
Oxide that reacts with water to form either an acid or a base

11. Properties of ionic substances

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12. What kind of bonds generally hold liquids together?
The solute is dissolved in the solvent.
NH2 functional group - name ends in -amide
Covalent
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

13. Carbonate ion
Soluble except when containing alkaline earth metals
Do not conduct electricity well
CO3²?
Covalent

14. Resonance structures
Light green
More active element replaces less active element in a compound.
1st group - most reactive metal family - react violently with water - create basic solutions
Same molecule - different electron pair positions

15. Compounds with 18 carbons
Defines shape of orbital
Solid at room temperature
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Mixture of silver and copper

16. Oxygen gas properties
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.
21% of atmosphere - colorless - odorless - supports combustion reactions
Pressure of mixture of gases equals some of individual gas pressures.
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

17. Compounds with 5-10 carbons
Liquid at room temperature - used to make gasoline and solvents
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Same formula - different structure
Excess oxygen

18. Gibb's Free Energy equation
Moles of solute / kg solvent
4.5 to 8.3 - Red to blue
DG = DH - TDS
COOH - ends in -oic acid

19. When a reaction is endothermic - the entropy is
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
No two electrons can have the same set of 4 quantum numbers
Increased
V1/T1 = V2/T2

20. Alkali metal properties
PO4³?
Gold
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
More active element replaces less active element in a compound.

21. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
A compound breaks into two parts

22. Hydrogen gas properties
DG = DH - TDS
Two reactants combine to form a single product
Most stable
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

23. Beta particle
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Increases left and down
DG = DH - TDS
Yes in thermo - no in electro

24. Ester
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Acid to water

25. How many joules are in a calorie?
Stronger
4.184
Low pressures - high temperatures
PO4³?

26. Sulfate ion
DH = bonds broken - bonds formed
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Blue
SO4²?

27. What kind of bonds generally hold gases together?
Orange
It is at equilibrium
Covalent
Green

28. Ionic solids
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Deadly - yellow-green - weapon
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
NH2 - ends in -amide

29. Radioactivity
Electrons are free to move through metal structure - high conductivity - ductile
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
COH functional group - name ends in -al
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

30. Amine group
Orange
Heat required to make a substance melt.
NH2 - ends in -amide
Limited oxygen

31. Carboxylic acid
Same molecule - different electron pair positions
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
NH4?
COOH functional group - name ends in oic acid

32. Acids with more oxygen atoms are
Stronger
2 bonding - 1 nonbonding
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Nonmetal oxides form acids - metal oxides form bases

33. F compounds are...
Mixture of iron and carbon
Soluble except when containing alkaline earth metals
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Two compound react to form two new compounds

34. Colligative properties
Blue
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Substance can act either as an acid or a base
Properties of solutions that depend on the number of particles per solvent molecule

35. Noble gas properties
Pressure of mixture of gases equals some of individual gas pressures.
4.5 to 8.3 - Red to blue
Most stable
Stronger

36. Chlorate ion
ClO3?
More active element replaces less active element in a compound.
NH2 functional group - name ends in -amide
Light green

37. What metal will react in hot water?
3.1 - 4.4 - red to yellow
Magnesium
Make up jet fuels and kerosene
Orange

38. List equivalent pressure values for mmHg - torr - atm - and Pa
Light green
Oxide that reacts with water to form either an acid or a base
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

39. Dalton's Law
Solid at room temperature
Limited oxygen
OH functional group - name ends in -ol
Pressure of mixture of gases equals some of individual gas pressures.

40. Color of excited Ba2+
Light green
Moles / L
Miscible with water - flammable - used as fuel - poisonous
Insoluble

41. Sulfide color: CdS
Mixture of tin - copper - bismuth - and antimony
Red
Bright yellow
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

42. SO4²? compounds are...
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Substance can act either as an acid or a base
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
3 bonding - 120° - sp² hybridization

43. Metallic bonds
3.1 - 4.4 - red to yellow
Electrons are free to move through metal structure - high conductivity - ductile
4.5 to 8.3 - Red to blue
4.184

44. Acetate ion
Bright yellow
C2H3O2?
Gases at room temperature - used for fuel
NO3?

45. Graham's Law
8.3 to 10.0 - colorless to pink
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Same element - different number of neutrons
3.1 - 4.4 - red to yellow

46. Ionic bond
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
More active element replaces less active element in a compound.
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

47. Chlorofluorocarbons
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Degrade the oxone layer
Mixture of iron and carbon

48. When the reaction is exothermic - the entropy is
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
R-O-R functional group - shorter chain ends in oxy - other is ane
Decreased
V1/T1 = V2/T2

49. Sigma bonds
Gas pressure = atm pressure + height of mercury
Stronger
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

50. Rare earth elements
Heat required to make a substance melt.
Extremely slow reactivity
Periods 8 and 9 - lanthanides and actinides
Lemon yellow