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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. Chlorate ion
Same element - different number of neutrons
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
ClO3?
CO - produced from incomplete combustion - very toxic

2. Sulfide color: Sb2S3
Diamond - graphite - amorphous - fullerenes
Emission of electromagnetic energy after beta - positron - or alpha decay
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Orange

3. Isotope
Bright yellow
Same element - different number of neutrons
Covalent
Black

4. Dalton's Law
Light green
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Involves water
Pressure of mixture of gases equals some of individual gas pressures.

5. Properties of bases
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Moles / L

6. Petroleum
Lemon yellow
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Gold
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

7. Carbon dioxide gas properties
Soluble except when containing alkaline earth metals
Heat required to make a substance melt.
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
C2H3O2?

8. Exceptions to the octet rule
6.0 to 7.6 - yellow to blue
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Gases at room temperature - used for fuel
Red

9. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Solid at room temperature
5 bonding - 90° and 120° - sp³d hybridization
Etching glass and frosting lightblubs

10. London dispersion forces
Disordered systems with higher entropies are favored
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Same molecule - different electron pair positions

11. Acetate ion
Yellow to orange
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
C2H3O2?
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

12. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
4.184
No two electrons can have the same set of 4 quantum numbers
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

13. Examples of strong electrolytes
Limited oxygen
NH4?
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Strong acids - strong bases - soluble salts

14. Ester
Most stable
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Orange
7th group - form salts - always exist as diatomic molecules - used in modern lighting

15. Hydrogen gas properties
Limited oxygen
Spin is +1/2 or -1/2 in an orbital
3 bonding - 120° - sp² hybridization
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

16. Sulfide color: As2S3
Emission of electromagnetic energy after beta - positron - or alpha decay
2 bonding - 1 nonbonding
Lemon yellow
R-O-R functional group - shorter chain ends in oxy - other is ane

17. Color of excited Li+ - Sr2+ - Ca2+
2 bonding - 1 nonbonding
DH = bonds broken - bonds formed
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Red

18. Pauli exclusion principle
6.0 to 7.6 - yellow to blue
A compound breaks into two parts
No two electrons can have the same set of 4 quantum numbers
Mixture of copper - zinc - and other metals

19. Solute vs. Solvent
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Oxide that reacts with water to form either an acid or a base
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
The solute is dissolved in the solvent.

20. Color of excited Fe3+
Blue
Green
Gold
Orange

21. Trigonal bipyramidal
Emission of electromagnetic energy after beta - positron - or alpha decay
5 bonding - 90° and 120° - sp³d hybridization
Disordered systems with higher entropies are favored
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

22. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
3 bonding - 120° - sp² hybridization
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Yes in thermo - no in electro
P1/V1 = P2/V2

23. Molarity
4 bonding - 109.5° - sp³ hybridization
Black
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Moles / L

24. List equivalent pressure values for mmHg - torr - atm - and Pa
Q = mcDT
Soluble except when containing Ag? - Hg2²? - or Pb²?
PO4³?
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

25. Brass
Mixture of copper and zinc
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Properties of solutions that depend on the number of particles per solvent molecule
Two atoms with the same number of electrons

26. Litmus: pH range and colors
Defines shape of orbital
4.5 to 8.3 - Red to blue
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
2nd group - fairly reactive - pastes are used in batteries

27. Amine
NH2 functional group - name ends in -amide
Increases left and down
Soluble
2 bonding - 180° - sp hybridization

28. What is the ideal gas law?
PV = nRT - R = .0821
M1V1 = M2V2
Gas pressure = atm pressure + height of mercury
Yellow to orange

29. Alchohols
OH functional group - name ends in -ol
Periods 8 and 9 - lanthanides and actinides
DG = DH - TDS
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

30. Isoelectronic
COOH - ends in -oic acid
Gas pressure = atm pressure - height of mercury
Two atoms with the same number of electrons
Limited oxygen

31. Phenolphthalein: pH range and colors
8.3 to 10.0 - colorless to pink
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

32. Color of Fe3+ solution
Red
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Yellow to orange

33. Properties of ionic substances

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34. Sulfide color: CdS
Two compound react to form two new compounds
Bright yellow
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
3.1 - 4.4 - red to yellow

35. Noble gas properties
yellow
Periods 8 and 9 - lanthanides and actinides
Increased
Most stable

36. Metallic bonds
Photography
Moles of solute / kg solvent
Electrons are free to move through metal structure - high conductivity - ductile
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

37. How can hydrogen be produced?
Soluble except when containing Ag? - Hg2²? - or Pb²?
Gas pressure = atm pressure + height of mercury
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Mixture of copper and zinc

38. Colloid
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Gold
Two atoms with the same number of electrons
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

39. Equation when using a barometer to calculate gas pressure.
Glass and plastic
Same molecule - different electron pair positions
Gas pressure = atm pressure - height of mercury
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

40. Add acid to water or water to acid
Light green
Pressure of mixture of gases equals some of individual gas pressures.
4 bonding - 109.5° - sp³ hybridization
Acid to water

41. Sterling silver
DG = DH - TDS
Mixture of silver and copper
2nd group - fairly reactive - pastes are used in batteries
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

42. Alkaline metal oxides are...
NH2 - ends in -amide
Heat required to make a substance melt.
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Classified as strong bases but not very soluble.

43. Halogen properties
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Increase right and up
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Properties of solutions that depend on the number of particles per solvent molecule

44. Compounds with 18 carbons
Q = mcDT
Limited oxygen
Solid at room temperature
Endothermic

45. Color of CrO7²? solution
3 bonding - 120° - sp² hybridization
Orange
Gas pressure = atm pressure - height of mercury
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

46. Nitrate ion
NO3?
Soluble
1st group - most reactive metal family - react violently with water - create basic solutions
Most stable

47. Sulfide color: ZnS
Degrade the oxone layer
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Mixture of silver and copper
White

48. Color of excited Ba2+
M1V1 = M2V2
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
DH = bonds broken - bonds formed
Light green

49. When the reaction is exothermic - the entropy is
Most stable
1st group - most reactive metal family - react violently with water - create basic solutions
Decreased
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

50. Covalent-network / atomic solids
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Same element - different number of neutrons
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
No