Test your basic knowledge |

SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Compounds with 1-4 carbons
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Covalent
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Gases at room temperature - used for fuel

2. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Orange
Properties of solutions that depend on the number of particles per solvent molecule
Insoluble
Miscible with water - flammable - used as fuel - poisonous

3. Azimuthal quantum number (l)
Glass and plastic
6 bonding - 90° - sp³d2² hybridization
6.0 to 7.6 - yellow to blue
Defines shape of orbital

4. Halogen properties
Moles of solute / kg solvent
2 bonding - 180° - sp hybridization
Gas pressure = atm pressure + height of mercury
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

5. Aldehydes
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Bright yellow
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
COH functional group - name ends in -al

6. Alchohols
Yes in thermo - no in electro
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
Red
OH functional group - name ends in -ol

7. What qualifies as a strong base?
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
NH4?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Classified as strong bases but not very soluble.

8. Color of excited Li+ - Sr2+ - Ca2+
Red
COOH - ends in -oic acid
Pressure of mixture of gases equals some of individual gas pressures.
Gases at room temperature - used for fuel

9. Hydrofluoric acid is used for
Yellow to orange
4.184
Etching glass and frosting lightblubs
Excess oxygen

10. Alkali Metals
1st group - most reactive metal family - react violently with water - create basic solutions
Covalent
Heat required to make a substance melt.
Q = mcDT

11. If G is positive - is the reaction spontaneous?
Bright yellow
No
Electrons are free to move through metal structure - high conductivity - ductile
OH functional group - name ends in -ol

12. Nonmetals
Orange
1st group - most reactive metal family - react violently with water - create basic solutions
Decreased
Do not conduct electricity well

13. Metallic bonds
21% of atmosphere - colorless - odorless - supports combustion reactions
Defines shape of orbital
Electrons are free to move through metal structure - high conductivity - ductile
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

14. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
Etching glass and frosting lightblubs
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Same molecule - different electron pair positions

15. Synthesis reaction
4.184
Green
Two reactants combine to form a single product
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

16. Sulfide color: ZnS
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
White
NH2 - ends in -amide
Excess oxygen

17. Sulfate ion
Increase right and up
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
OH - alcohols - name ends in ol
SO4²?

18. What kind of bonds generally hold liquids together?
Bright yellow
Covalent
Properties of solutions that depend on the number of particles per solvent molecule
Moles / L

19. Atomic radius trend
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Increases left and down
Yellow
Lemon yellow

20. Molality
Make up jet fuels and kerosene
Moles of solute / kg solvent
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
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

21. Color of excited Ba2+
Properties of solutions that depend on the number of particles per solvent molecule
PO4³?
Light green
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

22. Dipole-dipole forces (including hydrogen bonds)
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Soluble except when containing Ag? - Hg2²? - or Pb²?
Miscible with water - flammable - used as fuel - poisonous
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

23. If G is zero - what is happening in the reaction?
Emission of electromagnetic energy after beta - positron - or alpha decay
Red
It is at equilibrium
Orientation of orbital in space

24. Principal quantum number (n)
Low pressures - high temperatures
COH functional group - name ends in -al
Covalent
Energy level - as it increases electrons are less bound to the nucleus

25. Rare earth elements
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Covalent
Periods 8 and 9 - lanthanides and actinides
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

26. amphoteric
4.184
Substance can act either as an acid or a base
Mixture of iron and carbon
Soluble

27. Suspension
Limited oxygen
DH = bonds broken - bonds formed
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Blue

28. Color of MnO4? solution
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Purple
6.0 to 7.6 - yellow to blue
Q = mcDT

29. Amine group
NH2 - ends in -amide
Limited oxygen
Same element - different number of neutrons
Involves water

30. Alkali metal compounds and NH4? compounds are...
Heat required to make a substance melt.
Soluble
Two compound react to form two new compounds
4.184

31. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
COOH functional group - name ends in oic acid
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

32. Alpha particle
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
V1/T1 = V2/T2
Q = mcDT
Covalent

33. Colligative properties
Increase right and up
NH4?
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Properties of solutions that depend on the number of particles per solvent molecule

34. Radioactivity
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Substance can act either as an acid or a base
Mixture of copper - zinc - and other metals

35. What are the allotropic forms of sulfur?
Make up jet fuels and kerosene
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Black
More active element replaces less active element in a compound.

36. Silver bromide and silver iodide are used for
3 bonding - 1 nonbonding 107°
Substance can act either as an acid or a base
Photography
Moles / L

37. 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
Mixture of tin - copper - bismuth - and antimony
Heat required to make a substance melt.
NO3?

38. Ketone
Make up jet fuels and kerosene
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
yellow
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

39. Color of excited Fe3+
Photography
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Gold
The solute is dissolved in the solvent.

40. Solute vs. Solvent
Acid to water
The solute is dissolved in the solvent.
21% of atmosphere - colorless - odorless - supports combustion reactions
Strong acids - strong bases - soluble salts

41. Coal
Periods 8 and 9 - lanthanides and actinides
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
6 bonding - 90° - sp³d2² hybridization
Bright yellow

42. Acetate ion
C2H3O2?
Do not conduct electricity well
R-O-R functional group - shorter chain ends in oxy - other is ane
Light green

43. Trigonal planar
3 bonding - 120° - sp² hybridization
Substance can act either as an acid or a base
Yes
Oxide that reacts with water to form either an acid or a base

44. Petroleum
Heat required to make a substance melt.
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Two compound react to form two new compounds
Periods 8 and 9 - lanthanides and actinides

45. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Same element - different number of neutrons
NH4?
Spin is +1/2 or -1/2 in an orbital

46. Ethanol
Magnesium
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Soluble except when containing alkaline earth metals
Solid at room temperature

47. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Solid at room temperature
2 bonding - 180° - sp hybridization
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

48. Octahedral
Gases at room temperature - used for fuel
COH functional group - name ends in -al
6 bonding - 90° - sp³d2² hybridization
R-O-R functional group - shorter chain ends in oxy - other is ane

49. Hydrogen gas properties
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Orientation of orbital in space
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

50. Sulfide color: As2S3
The solute is dissolved in the solvent.
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Mixture of copper - zinc - and other metals
Lemon yellow