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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. Spin quantum number (ms)
Soluble
Insoluble
Spin is +1/2 or -1/2 in an orbital
Covalent

2. Single Replacement / displacement reaction
Covalent
More active element replaces less active element in a compound.
Gas pressure = atm pressure - height of mercury
Do not conduct electricity well

3. Color of Cu2+ solution
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Blue
A compound breaks into two parts
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

4. Colloid
Two reactants combine to form a single product
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
Two compound react to form two new compounds
Stronger

5. Colligative properties
Properties of solutions that depend on the number of particles per solvent molecule
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Endothermic
Gases at room temperature - used for fuel

6. Molarity
Diamond - graphite - amorphous - fullerenes
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Moles / L
Yes in thermo - no in electro

7. Molecular solids
NH2 functional group - name ends in -amide
CO3²?
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

8. Color of CrO7²? solution
No
Mixture of iron and carbon
Orange
Gold

9. SO4²? compounds are...
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
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Electrons are free to move through metal structure - high conductivity - ductile

10. Alkaline metal oxides are...
8.3 to 10.0 - colorless to pink
M1V1 = M2V2
Classified as strong bases but not very soluble.
COOH - ends in -oic acid

11. Nitrate ion
COH functional group - name ends in -al
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
NO3?
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.

12. Decomposition reaction
Increases left and down
Stronger
A compound breaks into two parts
Endothermic

13. Oxygen gas properties
Mixture of silver and copper
21% of atmosphere - colorless - odorless - supports combustion reactions
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
COOH functional group - name ends in oic acid

14. Positron emission
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
NH2 - ends in -amide
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
A compound breaks into two parts

15. Dilution equation
A compound breaks into two parts
Moles / L
M1V1 = M2V2
Insoluble

16. Trigonal pyramidal
3 bonding - 1 nonbonding 107°
COOH functional group - name ends in oic acid
Classified as strong bases but not very soluble.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

17. Brass
Mixture of copper and zinc
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
It is at equilibrium
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

18. What kind of bonds generally hold gases together?
Deadly - yellow-green - weapon
Disordered systems with higher entropies are favored
Blue
Covalent

19. Boyle's Law
P1/V1 = P2/V2
R-O-R functional group - shorter chain ends in oxy - other is ane
Red
COOH functional group - name ends in oic acid

20. Synthesis reaction
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
8.3 to 10.0 - colorless to pink
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Two reactants combine to form a single product

21. Octahedral
6 bonding - 90° - sp³d2² hybridization
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Soluble except when containing alkaline earth metals
Blue

22. Noble gases
Extremely slow reactivity
4.184
Lemon yellow
Covalent

23. What is the ideal gas law?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
A compound breaks into two parts
PV = nRT - R = .0821
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

24. What are the factors that affect reaction rate?
Two compound react to form two new compounds
R-O-R functional group - shorter chain ends in oxy - other is ane
SO4²?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

25. Alchohols
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
OH functional group - name ends in -ol
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
White

26. Boiling point elevation formula
NH2 functional group - name ends in -amide
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
2 bonding - 1 nonbonding
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

27. Gibb's Free Energy equation
Mixture of copper and zinc
Extremely slow reactivity
Same formula - different structure
DG = DH - TDS

28. Sulfate ion
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Glass and plastic
SO4²?
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

29. Sulfide color: ZnS
White
Substance can act either as an acid or a base
3.1 - 4.4 - red to yellow
4.184

30. Color of excited Ba2+
Gases at room temperature - used for fuel
Light green
Nonmetal oxides form acids - metal oxides form bases
8.3 to 10.0 - colorless to pink

31. Carbon monoxide
CO - produced from incomplete combustion - very toxic
It is at equilibrium
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
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

32. Gamma decay
Emission of electromagnetic energy after beta - positron - or alpha decay
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
ClO3?
Potassium - Calcium - Sodium

33. Color of CrO4²? solution
Yellow
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
COH functional group - name ends in -al
Light green

34. London dispersion forces
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Diamond - graphite - amorphous - fullerenes
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
5 bonding - 90° and 120° - sp³d hybridization

35. Cl - Br - and I compounds are...
Light green
Soluble except when containing Ag? - Hg2²? - or Pb²?
Moles of solute / kg solvent
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

36. Sulfide color: CuS - HgS - and PbS
Black
Covalent
1st group - most reactive metal family - react violently with water - create basic solutions
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

37. Acetate ion
8.3 to 10.0 - colorless to pink
3 bonding - 120° - sp² hybridization
Insoluble
C2H3O2?

38. Sulfide color: Sb2S3
Orange
7th group - form salts - always exist as diatomic molecules - used in modern lighting
NH2 functional group - name ends in -amide
Strong acids - strong bases - soluble salts

39. Equation when using a barometer to calculate gas pressure.
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
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
Electrons are free to move through metal structure - high conductivity - ductile

40. Combustion reaction
Substance can act either as an acid or a base
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
2nd group - fairly reactive - pastes are used in batteries
V1/T1 = V2/T2

41. Formula for calculating enthalpy change with bond energies
White
A compound breaks into two parts
DH = bonds broken - bonds formed
Degrade the oxone layer

42. Chlorofluorocarbons
Degrade the oxone layer
Yellow to orange
SO4²?
Classified as strong bases but not very soluble.

43. Noble gas properties
Most stable
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
21% of atmosphere - colorless - odorless - supports combustion reactions
1st group - most reactive metal family - react violently with water - create basic solutions

44. General Properties of Organic Compounds
5 bonding - 90° and 120° - sp³d hybridization
Gas pressure = atm pressure + height of mercury
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Etching glass and frosting lightblubs

45. Freezing point depression formula
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Nonmetal oxides form acids - metal oxides form bases
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

46. What kind of bonds generally hold liquids together?
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Covalent

47. Dalton's Law
Covalent
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Pressure of mixture of gases equals some of individual gas pressures.
No two electrons can have the same set of 4 quantum numbers

48. amphoteric
Substance can act either as an acid or a base
DG = DH - TDS
Insoluble
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

49. Examples of amorphous solids
Glass and plastic
Diamond - graphite - amorphous - fullerenes
Magnesium
7th group - form salts - always exist as diatomic molecules - used in modern lighting

50. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Diamond - graphite - amorphous - fullerenes
CO - produced from incomplete combustion - very toxic
Soluble
Blue