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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. Carbonate ion
Yes in thermo - no in electro
Increase right and up
CO3²?
Covalent

2. Charles' Law
The solute is dissolved in the solvent.
V1/T1 = V2/T2
Disordered systems with higher entropies are favored
Gas pressure = atm pressure + height of mercury

3. What metal will react in hot water?
Increase right and up
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Magnesium

4. Hydroxyl group
3.1 - 4.4 - red to yellow
OH - alcohols - name ends in ol
R-O-R functional group - shorter chain ends in oxy - other is ane
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

5. Is removing an electron an exothermic or endothermic process?
Substance can act either as an acid or a base
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Endothermic
21% of atmosphere - colorless - odorless - supports combustion reactions

6. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
NH2 functional group - name ends in -amide
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

7. Exceptions to the octet rule
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Mixture of tin - copper - bismuth - and antimony
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Same element - different number of neutrons

8. Hydrofluoric acid is used for
Do not conduct electricity well
Degrade the oxone layer
Etching glass and frosting lightblubs
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.

9. Pauli exclusion principle
Soluble except when containing alkaline earth metals
Glass and plastic
No two electrons can have the same set of 4 quantum numbers
Oxide that reacts with water to form either an acid or a base

10. Fission
A compound breaks into two parts
Gas pressure = atm pressure + height of mercury
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Properties of solutions that depend on the number of particles per solvent molecule

11. Magnetic quantum number (ml)
NH2 - ends in -amide
Extremely slow reactivity
Magnesium
Orientation of orbital in space

12. Transition metals
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Etching glass and frosting lightblubs
6 bonding - 90° - sp³d2² hybridization

13. Sulfide color: CuS - HgS - and PbS
Black
Degrade the oxone layer
Soluble except when containing Ag? - Hg2²? - or Pb²?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

14. What are the factors that affect reaction rate?
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
8.3 to 10.0 - colorless to pink
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

15. Combustion reaction
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Increases left and down
Defines shape of orbital
V1/T1 = V2/T2

16. Nonmetals
Covalent
Etching glass and frosting lightblubs
Do not conduct electricity well
Orange

17. Positron emission
3.1 - 4.4 - red to yellow
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

18. Aldehydes
Nonmetal oxides form acids - metal oxides form bases
COH functional group - name ends in -al
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Black

19. Decomposition reaction
A compound breaks into two parts
3 bonding - 1 nonbonding 107°
NH4?
Same element - different number of neutrons

20. Color of CrO7²? solution
Orange
Deadly - yellow-green - weapon
Increased
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

21. Sulfide color: ZnS
Bright yellow
Insoluble
White
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

22. Allotropic forms of carbon
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
NH4?
M1V1 = M2V2
Diamond - graphite - amorphous - fullerenes

23. Coal
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Mixture of silver and copper
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Mixture of copper - zinc - and other metals

24. Properties of molecular crystals and liquids

25. What is the ideal gas law?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Soluble
PV = nRT - R = .0821
Gold

26. Properties of bases
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Covalent
Yellow to orange
COH functional group - name ends in -al

27. What qualifies as a strong base?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Defines shape of orbital
No two electrons can have the same set of 4 quantum numbers
Soluble

28. Isomer
COOH - ends in -oic acid
Involves water
OH functional group - name ends in -ol
Same formula - different structure

29. amphoteric
Glass and plastic
Lemon yellow
Substance can act either as an acid or a base
M1V1 = M2V2

30. 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
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Two reactants combine to form a single product

31. Beta particle
M1V1 = M2V2
Mixture of silver and copper
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
1st group - most reactive metal family - react violently with water - create basic solutions

32. What kind of bonds generally hold gases together?
Same element - different number of neutrons
Covalent
It is at equilibrium
Red

33. What kind of bonds generally hold liquids together?
Covalent
COOH - ends in -oic acid
Pressure of mixture of gases equals some of individual gas pressures.
21% of atmosphere - colorless - odorless - supports combustion reactions

34. Trigonal planar
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
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
3 bonding - 120° - sp² hybridization

35. Molality
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Bright yellow
Moles of solute / kg solvent
Disordered systems with higher entropies are favored

36. Sterling silver
Mixture of silver and copper
Two reactants combine to form a single product
Mixture of copper and zinc
Solid at room temperature

37. Silver bromide and silver iodide are used for
Moles / L
NH2 functional group - name ends in -amide
Excess oxygen
Photography

38. 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
8.3 to 10.0 - colorless to pink
Same molecule - different electron pair positions
Two atoms with the same number of electrons

39. Oxides are insoluble and when reacted with water..
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
yellow
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Nonmetal oxides form acids - metal oxides form bases

40. Boyle's Law
Increases left and down
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.
4.5 to 8.3 - Red to blue
P1/V1 = P2/V2

41. Atomic radius trend
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
6 bonding - 90° - sp³d2² hybridization
Electrons are free to move through metal structure - high conductivity - ductile
Increases left and down

42. SO4²? compounds are...
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
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
6 bonding - 90° - sp³d2² hybridization
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

43. Fusion
NH2 - ends in -amide
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Blue

44. If G is positive - is the reaction spontaneous?
No
Bright yellow
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Strong acids - strong bases - soluble salts

45. Electronegativity
Two reactants combine to form a single product
Increase right and up
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Etching glass and frosting lightblubs

46. Sulfide color: As2S3
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Lemon yellow
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

47. Color of excited Na+
Black
Excess oxygen
yellow
No two electrons can have the same set of 4 quantum numbers

48. Color of Fe3+ solution
2 bonding - 180° - sp hybridization
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Yellow to orange
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

49. How can hydrogen be produced?
6.0 to 7.6 - yellow to blue
Energy level - as it increases electrons are less bound to the nucleus
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Limited oxygen

50. Nitrate ion
3 bonding - 120° - sp² hybridization
Yes in thermo - no in electro
Make up jet fuels and kerosene
NO3?