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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. Acetate ion
Diamond - graphite - amorphous - fullerenes
C2H3O2?
21% of atmosphere - colorless - odorless - supports combustion reactions
Oxide that reacts with water to form either an acid or a base

2. Molecular solids
3 bonding - 120° - sp² hybridization
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Strong acids - strong bases - soluble salts

3. Color of Fe3+ solution
Yellow to orange
6.0 to 7.6 - yellow to blue
Emission of electromagnetic energy after beta - positron - or alpha decay
CO3²?

4. Dalton's Law
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
Q = mcDT
Pressure of mixture of gases equals some of individual gas pressures.

5. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Mixture of iron and carbon
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Same molecule - different electron pair positions
Soluble

6. Single Replacement / displacement reaction
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Two atoms with the same number of electrons
R-O-R functional group - shorter chain ends in oxy - other is ane
More active element replaces less active element in a compound.

7. Halogen properties
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
No two electrons can have the same set of 4 quantum numbers
NH4?
Purple/pink

8. Compounds with 18 carbons
Solid at room temperature
Limited oxygen
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

9. Sulfide color: CuS - HgS - and PbS
Soluble
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
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
Black

10. Metallic bonds
2nd group - fairly reactive - pastes are used in batteries
Disordered systems with higher entropies are favored
DG = DH - TDS
Electrons are free to move through metal structure - high conductivity - ductile

11. Name the six strong acids
Gas pressure = atm pressure - height of mercury
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.
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Classified as strong bases but not very soluble.

12. Hydrolysis reaction
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Involves water
Two atoms with the same number of electrons
Emission of electromagnetic energy after beta - positron - or alpha decay

13. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Gas pressure = atm pressure + height of mercury
Insoluble
7th group - form salts - always exist as diatomic molecules - used in modern lighting

14. Color of Cu2+ solution
Spin is +1/2 or -1/2 in an orbital
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
COOH functional group - name ends in oic acid
Blue

15. Bent
Mixture of silver and copper
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
2 bonding - 1 nonbonding
Make up jet fuels and kerosene

16. Magnetic quantum number (ml)
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
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Orientation of orbital in space
2 bonding - 180° - sp hybridization

17. Ketone
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Green
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

18. Sulfate ion
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
SO4²?
PV = nRT - R = .0821
Soluble

19. Color of excited K+
Purple/pink
Orientation of orbital in space
Two compound react to form two new compounds
C2H3O2?

20. Formula for calculating enthalpy change with bond energies
Covalent
DH = bonds broken - bonds formed
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Increase right and up

21. Hydroxyl group
OH - alcohols - name ends in ol
ClO3?
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
NH4?

22. Incomplete combustion occurs when there is
Low pressures - high temperatures
Limited oxygen
Light green
Covalent

23. If G is positive - is the reaction spontaneous?
No
Purple
Limited oxygen
Nonmetal oxides form acids - metal oxides form bases

24. Alkali Metals
Mixture of copper - zinc - and other metals
Excess oxygen
1st group - most reactive metal family - react violently with water - create basic solutions
Two atoms with the same number of electrons

25. Anhydride
Oxide that reacts with water to form either an acid or a base
PO4³?
NO3?
Stronger

26. Oxides are insoluble and when reacted with water..
Nonmetal oxides form acids - metal oxides form bases
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Excess oxygen
Electrons are free to move through metal structure - high conductivity - ductile

27. What 3 metals will react with cold water?
No
NH2 functional group - name ends in -amide
Heat required to make a substance melt.
Potassium - Calcium - Sodium

28. Colloid
Endothermic
Spin is +1/2 or -1/2 in an orbital
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
Deadly - yellow-green - weapon

29. When are gases MOST ideal?
M1V1 = M2V2
Photography
NH2 - ends in -amide
Low pressures - high temperatures

30. Molarity
Moles / L
No
Insoluble
Soluble except when containing alkaline earth metals

31. Silver bromide and silver iodide are used for
Soluble except when containing Ag? - Hg2²? - or Pb²?
Same formula - different structure
Photography
PV = nRT - R = .0821

32. Covalent bond
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
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.
Disordered systems with higher entropies are favored

33. Nitrate ion
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
Red
NO3?
Purple/pink

34. Sterling silver
Emission of electromagnetic energy after beta - positron - or alpha decay
Two reactants combine to form a single product
Mixture of silver and copper
Defines shape of orbital

35. Isotope
Moles / L
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Same element - different number of neutrons
Do not conduct electricity well

36. Ethers
Emission of electromagnetic energy after beta - positron - or alpha decay
R-O-R functional group - shorter chain ends in oxy - other is ane
Yes
Mixture of tin - copper - bismuth - and antimony

37. Freezing point depression formula
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Extremely slow reactivity
Involves water
NH2 functional group - name ends in -amide

38. Electronegativity
Covalent
Decreased
Increase right and up
Same element - different number of neutrons

39. How can hydrogen be produced?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Two compound react to form two new compounds

40. Color of CrO7²? solution
Orange
Black
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Bright yellow

41. Aldehydes
COH functional group - name ends in -al
Mixture of silver and copper
Deadly - yellow-green - weapon
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

42. Metallic solids
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Mixture of silver and copper
6.0 to 7.6 - yellow to blue
Two compound react to form two new compounds

43. Equation when using a barometer to calculate gas pressure.
Gas pressure = atm pressure - height of mercury
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

44. pewter
Orange
Same formula - different structure
Mixture of tin - copper - bismuth - and antimony
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

45. Combustion reaction
Defines shape of orbital
White
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Spin is +1/2 or -1/2 in an orbital

46. What kind of bonds generally hold liquids together?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Covalent
Emission of electromagnetic energy after beta - positron - or alpha decay
Diamond - graphite - amorphous - fullerenes

47. What is the equation used for heat transfer problems?
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
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Q = mcDT
Same formula - different structure

48. Boiling point elevation formula
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Limited oxygen
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

49. Phenolphthalein: pH range and colors
Increased
Two atoms with the same number of electrons
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.
8.3 to 10.0 - colorless to pink

50. Properties of acids
Moles / L
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
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
CO3²?