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. Azimuthal quantum number (l)
Defines shape of orbital
Soluble
Properties of solutions that depend on the number of particles per solvent molecule
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

2. Sulfide color: Sb2S3
Orange
PO4³?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

3. Aldehydes
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
COH functional group - name ends in -al
Lemon yellow

4. Carboxylic acid
Blue
Mixture of copper and zinc
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
COOH functional group - name ends in oic acid

5. Dilution equation
M1V1 = M2V2
Yes in thermo - no in electro
Solid at room temperature
Moles of solute / kg solvent

6. Isomer
Gas pressure = atm pressure - height of mercury
Deadly - yellow-green - weapon
Same formula - different structure
Bright yellow

7. Ionic solids
6 bonding - 90° - sp³d2² hybridization
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
yellow
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

8. Sulfide color: ZnS
4.5 to 8.3 - Red to blue
Moles of solute / kg solvent
White
OH - alcohols - name ends in ol

9. Phenolphthalein: pH range and colors
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Bright yellow
8.3 to 10.0 - colorless to pink
Glass and plastic

10. Bent
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
2 bonding - 1 nonbonding
R-O-R functional group - shorter chain ends in oxy - other is ane

11. Ketone
21% of atmosphere - colorless - odorless - supports combustion reactions
Spin is +1/2 or -1/2 in an orbital
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
COOH functional group - name ends in oic acid

12. SO4²? compounds are...
Same element - different number of neutrons
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
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

13. Nonmetals
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Do not conduct electricity well
Moles / L
Electrons are free to move through metal structure - high conductivity - ductile

14. Radioactivity
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
4.5 to 8.3 - Red to blue
Q = mcDT

15. Color of CrO7²? solution
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Orange
Mixture of copper - zinc - and other metals
NH4?

16. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
3.1 - 4.4 - red to yellow
NH4?
Gas pressure = atm pressure + height of mercury
OH - alcohols - name ends in ol

17. Add acid to water or water to acid
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Acid to water
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
Oxide that reacts with water to form either an acid or a base

18. Halogen properties
Gas pressure = atm pressure - height of mercury
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

19. Trigonal planar
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
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
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
3 bonding - 120° - sp² hybridization

20. Examples of amorphous solids
A compound breaks into two parts
Glass and plastic
Emission of electromagnetic energy after beta - positron - or alpha decay
2 bonding - 180° - sp hybridization

21. Charles' Law
yellow
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
V1/T1 = V2/T2

22. What is the equation used for heat transfer problems?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Q = mcDT
Two compound react to form two new compounds
Mixture of tin - copper - bismuth - and antimony

23. Complete combustion occurs when there is
Excess oxygen
COH functional group - name ends in -al
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
COOH - ends in -oic acid

24. Sulfide color: As2S3
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Two reactants combine to form a single product
Lemon yellow
Yes in thermo - no in electro

25. Formula for calculating enthalpy change with bond energies
P1/V1 = P2/V2
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Insoluble
DH = bonds broken - bonds formed

26. What kind of bonds generally hold gases together?
Nonmetal oxides form acids - metal oxides form bases
Stronger
No
Covalent

27. Hydrolysis reaction
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
Potassium - Calcium - Sodium
Involves water

28. Amine group
NH2 - ends in -amide
CO3²?
Excess oxygen
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

29. Equation when using a barometer to calculate gas pressure.
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
P1/V1 = P2/V2
Gas pressure = atm pressure - height of mercury
Yes

30. When a reaction is endothermic - the entropy is
Increased
Stronger
4 bonding - 109.5° - sp³ hybridization
Purple/pink

31. Fusion
NH4?
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
V1/T1 = V2/T2

32. Double replacement reaction
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Two compound react to form two new compounds
Extremely slow reactivity
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

33. Transition metals
Etching glass and frosting lightblubs
Increases left and down
Covalent
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

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
NH2 functional group - name ends in -amide
Orange
M1V1 = M2V2

35. Halogens
Limited oxygen
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Increase right and up
Soluble except when containing alkaline earth metals

36. Ethers
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Properties of solutions that depend on the number of particles per solvent molecule
COH functional group - name ends in -al
R-O-R functional group - shorter chain ends in oxy - other is ane

37. Color of CrO4²? solution
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Yellow

38. Electron affinity
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Emission of electromagnetic energy after beta - positron - or alpha decay
3.1 - 4.4 - red to yellow
Nonmetal oxides form acids - metal oxides form bases

39. Trigonal bipyramidal
5 bonding - 90° and 120° - sp³d hybridization
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

40. Hydrogen gas properties
COOH functional group - name ends in oic acid
Two compound react to form two new compounds
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

41. Molarity
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
SO4²?
Moles / L
Same molecule - different electron pair positions

42. Allotropic forms of carbon
Diamond - graphite - amorphous - fullerenes
Two atoms with the same number of electrons
Soluble
4 bonding - 109.5° - sp³ hybridization

43. Sulfide color: CdS
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Bright yellow
Extremely slow reactivity
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

44. Properties of acids
M1V1 = M2V2
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
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
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

45. How can hydrogen be produced?
Increases left and down
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Gases at room temperature - used for fuel
Deadly - yellow-green - weapon

46. Principal quantum number (n)
Liquid at room temperature - used to make gasoline and solvents
Yes
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Energy level - as it increases electrons are less bound to the nucleus

47. Magnetic quantum number (ml)
NH4?
4 bonding - 109.5° - sp³ hybridization
Orientation of orbital in space
COOH functional group - name ends in oic acid

48. Spin quantum number (ms)
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
DH = bonds broken - bonds formed
Decreased
Spin is +1/2 or -1/2 in an orbital

49. Is removing an electron an exothermic or endothermic process?
Endothermic
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Same formula - different structure
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

50. Chlorine gas
Two atoms with the same number of electrons
Deadly - yellow-green - weapon
Classified as strong bases but not very soluble.
COOH - ends in -oic acid