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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. Color of excited Li+ - Sr2+ - Ca2+
Blue
Spin is +1/2 or -1/2 in an orbital
Lemon yellow
Red

2. Alkaline earth metals
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Orange
Miscible with water - flammable - used as fuel - poisonous
2nd group - fairly reactive - pastes are used in batteries

3. List equivalent pressure values for mmHg - torr - atm - and Pa
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Properties of solutions that depend on the number of particles per solvent molecule
Electrons are free to move through metal structure - high conductivity - ductile

4. Examples of strong electrolytes
Disordered systems with higher entropies are favored
Strong acids - strong bases - soluble salts
Most stable
Mixture of silver and copper

5. Metallic bonds
Electrons are free to move through metal structure - high conductivity - ductile
Mixture of copper - zinc - and other metals
Oxide that reacts with water to form either an acid or a base
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

6. Chlorofluorocarbons
2 bonding - 180° - sp hybridization
It is at equilibrium
Purple/pink
Degrade the oxone layer

7. Octahedral
6 bonding - 90° - sp³d2² hybridization
Low pressures - high temperatures
Covalent
Gases at room temperature - used for fuel

8. If G is zero - what is happening in the reaction?
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
2nd group - fairly reactive - pastes are used in batteries
More active element replaces less active element in a compound.
It is at equilibrium

9. Beta particle
Orange
DH = bonds broken - bonds formed
Q = mcDT
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

10. When a reaction is endothermic - the entropy is
Increased
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Mixture of silver and copper

11. Pauli exclusion principle
ClO3?
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
No two electrons can have the same set of 4 quantum numbers
Mixture of iron and carbon

12. Molarity
Moles / L
Orange
COH functional group - name ends in -al
8.3 to 10.0 - colorless to pink

13. Compounds with 12-18 carbons
Make up jet fuels and kerosene
3.1 - 4.4 - red to yellow
Light green
yellow

14. Tetrahedral
Soluble except when containing Ag? - Hg2²? - or Pb²?
Covalent
4 bonding - 109.5° - sp³ hybridization
Q = mcDT

15. Properties of molecular crystals and liquids

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16. Steel
Mixture of iron and carbon
The solute is dissolved in the solvent.
CO - produced from incomplete combustion - very toxic
Magnesium

17. Electronegativity
Mixture of copper - zinc - and other metals
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
3 bonding - 1 nonbonding 107°
Increase right and up

18. What kind of bonds generally hold gases together?
CO - produced from incomplete combustion - very toxic
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
More active element replaces less active element in a compound.
Covalent

19. Cl - Br - and I compounds are...
Q = mcDT
Soluble except when containing Ag? - Hg2²? - or Pb²?
Liquid at room temperature - used to make gasoline and solvents
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

20. Nonmetals
Magnesium
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Do not conduct electricity well
Purple/pink

21. Noble gases
Insoluble
Acid to water
2nd group - fairly reactive - pastes are used in batteries
Extremely slow reactivity

22. Ionization energy
Acid to water
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Miscible with water - flammable - used as fuel - poisonous

23. Hydroxyl group
Heat required to make a substance melt.
OH - alcohols - name ends in ol
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Low pressures - high temperatures

24. Sulfide color: CdS
No
Orientation of orbital in space
Bright yellow
Yellow

25. Color of excited Na+
Soluble
Mixture of copper and zinc
yellow
Black

26. Color of Cu2+ solution
Emission of electromagnetic energy after beta - positron - or alpha decay
Yellow
Limited oxygen
Blue

27. Isotope
4.184
Yes
Acid to water
Same element - different number of neutrons

28. Halogens
Liquid at room temperature - used to make gasoline and solvents
Two atoms with the same number of electrons
Soluble
7th group - form salts - always exist as diatomic molecules - used in modern lighting

29. Magnetic quantum number (ml)
OH - alcohols - name ends in ol
Orientation of orbital in space
8.3 to 10.0 - colorless to pink
4.184

30. Metallic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
6 bonding - 90° - sp³d2² hybridization
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Glass and plastic

31. Carboxylic acid group
Yellow
PV = nRT - R = .0821
Same formula - different structure
COOH - ends in -oic acid

32. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Same element - different number of neutrons
M1V1 = M2V2
OH - alcohols - name ends in ol
Soluble

33. SO4²? compounds are...
Stronger
Soluble
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

34. Molecular solids
4.5 to 8.3 - Red to blue
Glass and plastic
Yes
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

35. Bent
2 bonding - 1 nonbonding
Soluble
Low pressures - high temperatures
P1/V1 = P2/V2

36. Boiling point elevation formula
Bright yellow
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

37. General Properties of Organic Compounds
Two atoms with the same number of electrons
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

38. Nitrate ion
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
COH functional group - name ends in -al
NO3?
8.3 to 10.0 - colorless to pink

39. Ketone
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Yes
Defines shape of orbital

40. Atomic radius trend
Purple/pink
Increases left and down
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

41. Oxides are insoluble and when reacted with water..
CO - produced from incomplete combustion - very toxic
Stronger
Nonmetal oxides form acids - metal oxides form bases
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

42. Bromthymol blue: pH range and colors
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
NH4?
6.0 to 7.6 - yellow to blue
Increase right and up

43. Is removing an electron an exothermic or endothermic process?
Endothermic
Light green
P1/V1 = P2/V2
Potassium - Calcium - Sodium

44. Sulfate ion
Lemon yellow
NH2 functional group - name ends in -amide
Oxide that reacts with water to form either an acid or a base
SO4²?

45. Carboxylic acid
COOH functional group - name ends in oic acid
Orientation of orbital in space
3 bonding - 120° - sp² hybridization
Two atoms with the same number of electrons

46. Alkaline metal oxides are...
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
3 bonding - 1 nonbonding 107°
Classified as strong bases but not very soluble.
Most stable

47. Charles' Law
3 bonding - 120° - sp² hybridization
V1/T1 = V2/T2
Most stable
PO4³?

48. Combustion reaction
Covalent
Oxide that reacts with water to form either an acid or a base
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

49. Color of CrO4²? solution
Lemon yellow
Yes in thermo - no in electro
Yellow
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

50. Electron affinity
Gases at room temperature - used for fuel
Red
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Periods 8 and 9 - lanthanides and actinides