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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. Properties of acids
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
Substance can act either as an acid or a base
6 bonding - 90° - sp³d2² hybridization
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

2. Isoelectronic
Soluble
Same molecule - different electron pair positions
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Two atoms with the same number of electrons

3. Incomplete combustion occurs when there is
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Limited oxygen
Liquid at room temperature - used to make gasoline and solvents
CO3²?

4. Boyle's Law
Yes
Mixture of copper - zinc - and other metals
P1/V1 = P2/V2
PO4³?

5. When are gases MOST ideal?
Soluble except when containing alkaline earth metals
CO - produced from incomplete combustion - very toxic
Low pressures - high temperatures
Mixture of copper - zinc - and other metals

6. Color of CrO7²? solution
Light green
Orange
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

7. Coal
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Moles of solute / kg solvent
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

8. Ester
1st group - most reactive metal family - react violently with water - create basic solutions
No
Purple/pink
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

9. What kind of bonds generally hold liquids together?
Covalent
DH = bonds broken - bonds formed
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
No

10. If G is positive - is the reaction spontaneous?
No
Covalent
SO4²?
3 bonding - 120° - sp² hybridization

11. Molecular solids
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Gold
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

12. Compounds with 12-18 carbons
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Make up jet fuels and kerosene
NH4?
3.1 - 4.4 - red to yellow

13. Metallic solids
2 bonding - 180° - sp hybridization
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
The solute is dissolved in the solvent.
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

14. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Gas pressure = atm pressure - height of mercury
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
Soluble
Two reactants combine to form a single product

15. Spin quantum number (ms)
Spin is +1/2 or -1/2 in an orbital
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

16. What are the factors that affect reaction rate?
Stronger
Electrons are free to move through metal structure - high conductivity - ductile
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
R-O-R functional group - shorter chain ends in oxy - other is ane

17. Carbon dioxide gas properties
Deadly - yellow-green - weapon
2 bonding - 180° - sp hybridization
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Substance can act either as an acid or a base

18. Color of Ni2+ solution
Green
Soluble
Endothermic
Blue-green

19. Examples of amorphous solids
Glass and plastic
3.1 - 4.4 - red to yellow
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
No two electrons can have the same set of 4 quantum numbers

20. Sterling silver
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Mixture of silver and copper
Moles / L
Two compound react to form two new compounds

21. Double replacement reaction
4.5 to 8.3 - Red to blue
Two compound react to form two new compounds
Q = mcDT
Soluble except when containing Ag? - Hg2²? - or Pb²?

22. Gamma decay
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
3.1 - 4.4 - red to yellow
Emission of electromagnetic energy after beta - positron - or alpha decay

23. When a reaction is endothermic - the entropy is
Endothermic
Two atoms with the same number of electrons
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Increased

24. Electron affinity
Yes in thermo - no in electro
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Red

25. Alchohols
OH functional group - name ends in -ol
ClO3?
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Black

26. Silver bromide and silver iodide are used for
Photography
More active element replaces less active element in a compound.
Pressure of mixture of gases equals some of individual gas pressures.
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

27. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Gas pressure = atm pressure + height of mercury
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
CO - produced from incomplete combustion - very toxic
Red

28. SO4²? compounds are...
4 bonding - 109.5° - sp³ hybridization
CO - produced from incomplete combustion - very toxic
NH4?
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

29. Litmus: pH range and colors
OH functional group - name ends in -ol
4.5 to 8.3 - Red to blue
Moles / L
Mixture of tin - copper - bismuth - and antimony

30. Amine
Spin is +1/2 or -1/2 in an orbital
NH2 functional group - name ends in -amide
8.3 to 10.0 - colorless to pink
2nd group - fairly reactive - pastes are used in batteries

31. Petroleum
2nd group - fairly reactive - pastes are used in batteries
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Nonmetal oxides form acids - metal oxides form bases
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

32. What is the equation used for heat transfer problems?
M1V1 = M2V2
21% of atmosphere - colorless - odorless - supports combustion reactions
Insoluble
Q = mcDT

33. Alkali Metals
Yes in thermo - no in electro
Mixture of copper - zinc - and other metals
CO - produced from incomplete combustion - very toxic
1st group - most reactive metal family - react violently with water - create basic solutions

34. Dalton's Law
Diamond - graphite - amorphous - fullerenes
Pressure of mixture of gases equals some of individual gas pressures.
SO4²?
PV = nRT - R = .0821

35. When the reaction is exothermic - the entropy is
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Decreased
Soluble except when containing alkaline earth metals
More active element replaces less active element in a compound.

36. Chlorofluorocarbons
Degrade the oxone layer
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Insoluble
Red

37. Resonance structures
Lemon yellow
2 bonding - 1 nonbonding
Moles / L
Same molecule - different electron pair positions

38. Atomic radius trend
Mixture of copper and zinc
2 bonding - 180° - sp hybridization
Increases left and down
Two atoms with the same number of electrons

39. Compounds with 1-4 carbons
R-O-R functional group - shorter chain ends in oxy - other is ane
Gases at room temperature - used for fuel
Mixture of copper - zinc - and other metals
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

40. Alkaline metal oxides are...
Classified as strong bases but not very soluble.
Increase right and up
Red
NH2 - ends in -amide

41. Hydrolysis reaction
Soluble
Insoluble
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Involves water

42. Decomposition reaction
2 bonding - 180° - sp hybridization
A compound breaks into two parts
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Oxide that reacts with water to form either an acid or a base

43. What are the allotropic forms of sulfur?
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
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Yes
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

44. Rare earth elements
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Yellow
Periods 8 and 9 - lanthanides and actinides

45. Color of CrO4²? solution
Two reactants combine to form a single product
Green
NO3?
Yellow

46. Fission
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Photography

47. Equation when using a barometer to calculate gas pressure.
Mixture of copper - zinc - and other metals
Two reactants combine to form a single product
2 bonding - 180° - sp hybridization
Gas pressure = atm pressure - height of mercury

48. Fusion
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Emission of electromagnetic energy after beta - positron - or alpha decay
Gases at room temperature - used for fuel
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

49. Synthesis reaction
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Photography
Bright yellow
Two reactants combine to form a single product

50. Color of excited Fe3+
Insoluble
Two compound react to form two new compounds
Gold
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2