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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. Color of CrO7²? solution
Orange
COH functional group - name ends in -al
It is at equilibrium
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

2. If G is positive - is the reaction spontaneous?
No
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
CO3²?
The solute is dissolved in the solvent.

3. Fusion
Properties of solutions that depend on the number of particles per solvent molecule
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Yes
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

4. Ester
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
CO - produced from incomplete combustion - very toxic
COOH - ends in -oic acid

5. SO4²? compounds are...
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Covalent
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

6. Fission
Bright yellow
Mixture of copper and zinc
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Glass and plastic

7. Pi bonds
NH2 functional group - name ends in -amide
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
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
Liquid at room temperature - used to make gasoline and solvents

8. Combustion reaction
Strong acids - strong bases - soluble salts
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

9. What are the allotropic forms of sulfur?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
White
Same molecule - different electron pair positions
Soluble

10. Boyle's Law
Moles of solute / kg solvent
Orange
Miscible with water - flammable - used as fuel - poisonous
P1/V1 = P2/V2

11. Sulfide color: ZnS
ClO3?
White
Blue-green
21% of atmosphere - colorless - odorless - supports combustion reactions

12. Methyl orange: pH range and colors
8.3 to 10.0 - colorless to pink
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Covalent
3.1 - 4.4 - red to yellow

13. F compounds are...
Degrade the oxone layer
Moles / L
V1/T1 = V2/T2
Soluble except when containing alkaline earth metals

14. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Same element - different number of neutrons
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Gas pressure = atm pressure + height of mercury
COH functional group - name ends in -al

15. Charles' Law
COH functional group - name ends in -al
V1/T1 = V2/T2
PV = nRT - R = .0821
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

16. Phenolphthalein: pH range and colors
Gas pressure = atm pressure + height of mercury
It is at equilibrium
Extremely slow reactivity
8.3 to 10.0 - colorless to pink

17. What are the factors that affect reaction rate?
Gas pressure = atm pressure - height of mercury
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
yellow
A compound breaks into two parts

18. Ethers
4.5 to 8.3 - Red to blue
R-O-R functional group - shorter chain ends in oxy - other is ane
Decreased
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

19. Properties of acids
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
Diamond - graphite - amorphous - fullerenes
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Potassium - Calcium - Sodium

20. Oxides are insoluble and when reacted with water..
NH2 functional group - name ends in -amide
Nonmetal oxides form acids - metal oxides form bases
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

21. Trigonal bipyramidal
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Involves water
Do not conduct electricity well
5 bonding - 90° and 120° - sp³d hybridization

22. Isoelectronic
Two atoms with the same number of electrons
Photography
Orange
C2H3O2?

23. Acetate ion
2 bonding - 1 nonbonding
Red
C2H3O2?
Light green

24. Equation when using a barometer to calculate gas pressure.
Electrons are free to move through metal structure - high conductivity - ductile
Gas pressure = atm pressure - height of mercury
Pressure of mixture of gases equals some of individual gas pressures.
NH4?

25. Carbon dioxide gas properties
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.
5 bonding - 90° and 120° - sp³d hybridization
DG = DH - TDS

26. Chlorate ion
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Lemon yellow
ClO3?
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

27. Octahedral
NO3?
6 bonding - 90° - sp³d2² hybridization
Acid to water
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

28. Tetrahedral
Lemon yellow
4 bonding - 109.5° - sp³ hybridization
Gas pressure = atm pressure + height of mercury
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

29. Sulfide color: CdS
yellow
Covalent
Bright yellow
Black

30. Metallic solids
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
PV = nRT - R = .0821
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

31. Compounds with 12-18 carbons
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Make up jet fuels and kerosene
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Two atoms with the same number of electrons

32. Synthesis reaction
Insoluble
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Two reactants combine to form a single product
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

33. Properties of ionic substances

34. Principal quantum number (n)
4.5 to 8.3 - Red to blue
6 bonding - 90° - sp³d2² hybridization
Degrade the oxone layer
Energy level - as it increases electrons are less bound to the nucleus

35. Isomer
Degrade the oxone layer
Decreased
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Same formula - different structure

36. What is the ideal gas law?
PV = nRT - R = .0821
2nd group - fairly reactive - pastes are used in batteries
Excess oxygen
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

37. Alkali metal properties
Bright yellow
4.184
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Increases left and down

38. Hydrogen gas properties
Gold
Insoluble
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

39. Gamma decay
Periods 8 and 9 - lanthanides and actinides
Magnesium
Emission of electromagnetic energy after beta - positron - or alpha decay
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

40. Chlorofluorocarbons
Black
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Properties of solutions that depend on the number of particles per solvent molecule
Degrade the oxone layer

41. How many joules are in a calorie?
Mixture of silver and copper
4.184
Q = mcDT
COOH - ends in -oic acid

42. If G is negative - is the reaction spontaneous?
Yes
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Gas pressure = atm pressure - height of mercury
Covalent

43. Sulfide color: Sb2S3
Orange
ClO3?
Emission of electromagnetic energy after beta - positron - or alpha decay
Strong acids - strong bases - soluble salts

44. Complete combustion occurs when there is
Excess oxygen
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
3 bonding - 120° - sp² hybridization
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

45. Amine group
Liquid at room temperature - used to make gasoline and solvents
NH2 - ends in -amide
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
White

46. Compounds with 1-4 carbons
Low pressures - high temperatures
Purple/pink
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Gases at room temperature - used for fuel

47. Add acid to water or water to acid
Acid to water
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Soluble except when containing alkaline earth metals
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

48. Dilution equation
Q = mcDT
4.5 to 8.3 - Red to blue
M1V1 = M2V2
21% of atmosphere - colorless - odorless - supports combustion reactions

49. Decomposition reaction
No two electrons can have the same set of 4 quantum numbers
A compound breaks into two parts
CO - produced from incomplete combustion - very toxic
P1/V1 = P2/V2

50. Coal
Mixture of silver and copper
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Same formula - different structure