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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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1. Supersaturated solution
Mixture of iron and carbon
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
More active element replaces less active element in a compound.
Mixture of copper and zinc

2. Amine
Disordered systems with higher entropies are favored
Deadly - yellow-green - weapon
Soluble
NH2 functional group - name ends in -amide

3. Freezing point depression formula
Soluble
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
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

4. Nitrate ion
Acid to water
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
NO3?

5. Is removing an electron an exothermic or endothermic process?
Endothermic
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Gold
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.

6. What are the allotropic forms of sulfur?
6 bonding - 90° - sp³d2² hybridization
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
White
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

7. Linear
DG = DH - TDS
yellow
8.3 to 10.0 - colorless to pink
2 bonding - 180° - sp hybridization

8. What are the factors that affect reaction rate?
NH2 - ends in -amide
Solid at room temperature
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Miscible with water - flammable - used as fuel - poisonous

9. Color of excited Fe3+
Energy level - as it increases electrons are less bound to the nucleus
White
Soluble except when containing Ag? - Hg2²? - or Pb²?
Gold

10. Methanol
Orange
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Miscible with water - flammable - used as fuel - poisonous
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

11. Formula for calculating enthalpy change with bond energies
Two reactants combine to form a single product
Increases left and down
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
DH = bonds broken - bonds formed

12. If G is negative - is the reaction spontaneous?
Yes
4.5 to 8.3 - Red to blue
3.1 - 4.4 - red to yellow
Diamond - graphite - amorphous - fullerenes

13. Compounds with 12-18 carbons
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Make up jet fuels and kerosene
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

14. Fission
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Same molecule - different electron pair positions
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)

15. Pi bonds
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Same formula - different structure
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
6 bonding - 90° - sp³d2² hybridization

16. Carboxylic acid group
No
COOH - ends in -oic acid
Gas pressure = atm pressure - height of mercury
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

17. General Properties of Organic Compounds
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
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
OH functional group - name ends in -ol

18. Name the six strong acids
PV = nRT - R = .0821
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Oxide that reacts with water to form either an acid or a base

19. Hydrogen gas properties
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
CO3²?
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

20. Sigma bonds
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
PO4³?
Blue-green
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

21. Noble gas properties
OH functional group - name ends in -ol
Most stable
NO3?
6 bonding - 90° - sp³d2² hybridization

22. Decomposition reaction
Yellow
Solid at room temperature
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
A compound breaks into two parts

23. Covalent-network / atomic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
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
3.1 - 4.4 - red to yellow
Most stable

24. If G is positive - is the reaction spontaneous?
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
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
No

25. Color of excited K+
COOH functional group - name ends in oic acid
Purple/pink
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Insoluble

26. Silver bromide and silver iodide are used for
Lemon yellow
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Photography

27. Coal
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
21% of atmosphere - colorless - odorless - supports combustion reactions
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

28. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Insoluble
DG = DH - TDS
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
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

29. Graham's Law
Substance can act either as an acid or a base
C2H3O2?
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
OH - alcohols - name ends in ol

30. Sterling silver
Electrons are free to move through metal structure - high conductivity - ductile
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Acid to water
Mixture of silver and copper

31. Alkali metal properties
C2H3O2?
Endothermic
A compound breaks into two parts
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

32. Color of MnO4? solution
Purple
Yellow
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Properties of solutions that depend on the number of particles per solvent molecule

33. Acids with more oxygen atoms are
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Mixture of iron and carbon
Stronger

34. Sulfide color: As2S3
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Lemon yellow
Red
Increased

35. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Two compound react to form two new compounds
Purple

36. Compounds with 18 carbons
Bright yellow
Solid at room temperature
NH2 - ends in -amide
Excess oxygen

37. Suspension
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
2 bonding - 180° - sp hybridization
CO3²?
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

38. How can hydrogen be produced?
Spin is +1/2 or -1/2 in an orbital
1st group - most reactive metal family - react violently with water - create basic solutions
R-O-R functional group - shorter chain ends in oxy - other is ane
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

39. List equivalent pressure values for mmHg - torr - atm - and Pa
Green
Bright yellow
Same formula - different structure
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

40. What qualifies as a strong base?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Blue
Increased

41. Azimuthal quantum number (l)
Same element - different number of neutrons
Involves water
More active element replaces less active element in a compound.
Defines shape of orbital

42. Complete combustion occurs when there is
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
3.1 - 4.4 - red to yellow
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Excess oxygen

43. Trigonal planar
The solute is dissolved in the solvent.
Solid at room temperature
3 bonding - 120° - sp² hybridization
2 bonding - 180° - sp hybridization

44. Anhydride
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Oxide that reacts with water to form either an acid or a base
CO - produced from incomplete combustion - very toxic
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.

45. F compounds are...
OH - alcohols - name ends in ol
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Gas pressure = atm pressure + height of mercury
Soluble except when containing alkaline earth metals

46. Gamma decay
4 bonding - 109.5° - sp³ hybridization
Emission of electromagnetic energy after beta - positron - or alpha decay
6.0 to 7.6 - yellow to blue
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

47. SO4²? compounds are...
Limited oxygen
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Classified as strong bases but not very soluble.
Blue

48. Synthesis reaction
P1/V1 = P2/V2
Two reactants combine to form a single product
Miscible with water - flammable - used as fuel - poisonous
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

49. Alkali Metals
1st group - most reactive metal family - react violently with water - create basic solutions
Etching glass and frosting lightblubs
No
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

50. What kind of bonds generally hold gases together?
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Covalent
DG = DH - TDS

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SAT Subject Test: Chemistry

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