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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. Transition metals
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
M1V1 = M2V2
COOH functional group - name ends in oic acid
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

2. Silver bromide and silver iodide are used for
Potassium - Calcium - Sodium
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Photography
Substance can act either as an acid or a base

3. Acetate ion
3.1 - 4.4 - red to yellow
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Blue
C2H3O2?

4. Color of CrO4²? solution
Yellow
NH2 - ends in -amide
Mixture of copper and zinc
Involves water

5. List equivalent pressure values for mmHg - torr - atm - and 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
Orientation of orbital in space
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
2nd group - fairly reactive - pastes are used in batteries

6. Chlorofluorocarbons
Degrade the oxone layer
Green
Spin is +1/2 or -1/2 in an orbital
Electrons are free to move through metal structure - high conductivity - ductile

7. Charles' Law
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
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
V1/T1 = V2/T2
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

8. Alkali metal compounds and NH4? compounds are...
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
Soluble except when containing alkaline earth metals
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Soluble

9. If G is zero - what is happening in the reaction?
Increased
It is at equilibrium
OH functional group - name ends in -ol
DG = DH - TDS

10. Gibb's Free Energy equation
3.1 - 4.4 - red to yellow
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Light green
DG = DH - TDS

11. Solute vs. Solvent
Orientation of orbital in space
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
The solute is dissolved in the solvent.
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent

12. Hydrofluoric acid is used for
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Etching glass and frosting lightblubs
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Green

13. What kind of bonds generally hold gases together?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Diamond - graphite - amorphous - fullerenes
Covalent

14. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
CO3²?
6.0 to 7.6 - yellow to blue

15. Complete combustion occurs when there is
Orientation of orbital in space
Excess oxygen
Make up jet fuels and kerosene
2 bonding - 180° - sp hybridization

16. Colligative properties
Properties of solutions that depend on the number of particles per solvent molecule
NO3?
ClO3?
Black

17. Alkaline metal oxides are...
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Classified as strong bases but not very soluble.
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Disordered systems with higher entropies are favored

18. Define heat of fusion.
Heat required to make a substance melt.
Involves water
A compound breaks into two parts
Most stable

19. Anhydride
NH4?
M1V1 = M2V2
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Oxide that reacts with water to form either an acid or a base

20. Sulfide color: ZnS
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
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
White
Magnesium

21. Rare earth elements
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Potassium - Calcium - Sodium
Periods 8 and 9 - lanthanides and actinides
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

22. Combustion reaction
Make up jet fuels and kerosene
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
More active element replaces less active element in a compound.

23. Ionic solids
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Orange

24. Color of excited Ba2+
NO3?
COH functional group - name ends in -al
Covalent
Light green

25. Carbon dioxide gas properties
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.
Yes
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
7th group - form salts - always exist as diatomic molecules - used in modern lighting

26. Isotope
Same element - different number of neutrons
NH2 - ends in -amide
2 bonding - 1 nonbonding
4 bonding - 109.5° - sp³ hybridization

27. Properties of molecular crystals and liquids

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28. Sulfate ion
Endothermic
Same element - different number of neutrons
SO4²?
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.

29. Nitrate ion
Solid at room temperature
Do not conduct electricity well
NO3?
Soluble except when containing Ag? - Hg2²? - or Pb²?

30. Color of MnO4? solution
Moles of solute / kg solvent
Purple
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

31. Ionization energy
Yes in thermo - no in electro
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
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Periods 8 and 9 - lanthanides and actinides

32. Isoelectronic
Energy level - as it increases electrons are less bound to the nucleus
Soluble
Two atoms with the same number of electrons
Etching glass and frosting lightblubs

33. Halogens
DH = bonds broken - bonds formed
SO4²?
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Lemon yellow

34. Carboxylic 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
COOH functional group - name ends in oic acid
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

35. How many joules are in a calorie?
COOH functional group - name ends in oic acid
4.184
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

36. Color of excited Fe3+
6 bonding - 90° - sp³d2² hybridization
Purple/pink
Gold
Orange

37. Sulfide color: Sb2S3
Orange
Yellow to orange
Green
Mixture of copper and zinc

38. Aldehydes
COH functional group - name ends in -al
Electrons are free to move through metal structure - high conductivity - ductile
SO4²?
Photography

39. What 3 metals will react with cold water?
Moles of solute / kg solvent
Potassium - Calcium - Sodium
The solute is dissolved in the solvent.
Same formula - different structure

40. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Insoluble
yellow
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Lemon yellow

41. Metallic solids
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Increases left and down
Photography
Two compound react to form two new compounds

42. Molecular solids
1st group - most reactive metal family - react violently with water - create basic solutions
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

43. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Energy level - as it increases electrons are less bound to the nucleus
Mixture of silver and copper
1st group - most reactive metal family - react violently with water - create basic solutions

44. Sulfide color: As2S3
Photography
Covalent
Lemon yellow
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

45. Steel
M1V1 = M2V2
Gas pressure = atm pressure + height of mercury
Mixture of iron and carbon
CO3²?

46. Color of excited Na+
Same molecule - different electron pair positions
Covalent
yellow
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

47. Alkaline earth metals
Orange
2nd group - fairly reactive - pastes are used in batteries
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
PV = nRT - R = .0821

48. 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
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

49. What is the equation used for heat transfer problems?
Orientation of orbital in space
Q = mcDT
Black
Soluble

50. Electron affinity
It is at equilibrium
Emission of electromagnetic energy after beta - positron - or alpha decay
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Extremely slow reactivity