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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. SO4²? compounds are...
Mixture of silver and copper
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Soluble except when containing Ag? - Hg2²? - or Pb²?
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

2. Fission
Purple/pink
Yellow
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Two compound react to form two new compounds

3. Alkaline metal oxides are...
Blue-green
Classified as strong bases but not very soluble.
2 bonding - 1 nonbonding
OH - alcohols - name ends in ol

4. Complete combustion occurs when there is
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
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Excess oxygen
Blue-green

5. amphoteric
Substance can act either as an acid or a base
Magnesium
Decreased
Degrade the oxone layer

6. Anhydride
4.5 to 8.3 - Red to blue
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Oxide that reacts with water to form either an acid or a base
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

7. Amine group
Decreased
NH2 - ends in -amide
Same element - different number of neutrons
NH2 functional group - name ends in -amide

8. Transition metals
Do not conduct electricity well
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Soluble
OH - alcohols - name ends in ol

9. Alkaline earth metals
Increased
Q = mcDT
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
2nd group - fairly reactive - pastes are used in batteries

10. List equivalent pressure values for mmHg - torr - atm - and Pa
Blue-green
Glass and plastic
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
1st group - most reactive metal family - react violently with water - create basic solutions

11. Add acid to water or water to acid
OH - alcohols - name ends in ol
DG = DH - TDS
Acid to water
NH2 functional group - name ends in -amide

12. What qualifies as a strong base?
A compound breaks into two parts
Mixture of copper and zinc
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

13. Methanol
OH functional group - name ends in -ol
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Miscible with water - flammable - used as fuel - poisonous
Degrade the oxone layer

14. Exceptions to the octet rule
NH4?
Blue
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
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

15. Color of excited K+
Purple/pink
Red
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

16. Color of CrO7²? solution
COH functional group - name ends in -al
NH4?
Orange
Emission of electromagnetic energy after beta - positron - or alpha decay

17. What is the second law of thermodynamics?
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
4.5 to 8.3 - Red to blue
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Disordered systems with higher entropies are favored

18. Hydrofluoric acid is used for
Etching glass and frosting lightblubs
4.5 to 8.3 - Red to blue
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Soluble except when containing alkaline earth metals

19. General Properties of Organic Compounds
Mixture of silver and copper
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

20. Alkali metal properties
Limited oxygen
Liquid at room temperature - used to make gasoline and solvents
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
OH functional group - name ends in -ol

21. Ethers
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Purple
R-O-R functional group - shorter chain ends in oxy - other is ane
DH = bonds broken - bonds formed

22. Properties of bases
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
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Degrade the oxone layer

23. Alpha particle
Oxide that reacts with water to form either an acid or a base
Strong acids - strong bases - soluble salts
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
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

24. Carbonate ion
Moles / L
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Excess oxygen
CO3²?

25. Double replacement reaction
ClO3?
2 bonding - 180° - sp hybridization
Two compound react to form two new compounds
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

26. Trigonal pyramidal
Yes
3 bonding - 1 nonbonding 107°
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Soluble except when containing Ag? - Hg2²? - or Pb²?

27. Molarity
Soluble
Gold
3 bonding - 120° - sp² hybridization
Moles / L

28. Bent
2 bonding - 1 nonbonding
It is at equilibrium
PO4³?
Excess oxygen

29. Dalton's Law
Pressure of mixture of gases equals some of individual gas pressures.
1st group - most reactive metal family - react violently with water - create basic solutions
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
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

30. Charles' Law
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
COH functional group - name ends in -al
V1/T1 = V2/T2
No

31. Litmus: pH range and colors
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
4.5 to 8.3 - Red to blue
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
yellow

32. Carbon monoxide
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
3.1 - 4.4 - red to yellow
Green
CO - produced from incomplete combustion - very toxic

33. Magnetic quantum number (ml)
Low pressures - high temperatures
Soluble except when containing alkaline earth metals
Orientation of orbital in space
5 bonding - 90° and 120° - sp³d hybridization

34. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
Purple
NH4?
Stronger

35. Hydrogen gas properties
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Magnesium
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
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

36. Positron emission
Electrons are free to move through metal structure - high conductivity - ductile
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Excess oxygen
NH2 - ends in -amide

37. If G is negative - is the reaction spontaneous?
3 bonding - 1 nonbonding 107°
8.3 to 10.0 - colorless to pink
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Yes

38. Halogen properties
Red
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Substance can act either as an acid or a base
Decreased

39. Graham's Law
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Orange
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

40. Allotropic forms of carbon
Insoluble
Diamond - graphite - amorphous - fullerenes
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

41. Sulfide color: CdS
Periods 8 and 9 - lanthanides and actinides
Soluble except when containing alkaline earth metals
Bright yellow
Photography

42. Color of excited Fe3+
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Mixture of copper and zinc
NH2 - ends in -amide
Gold

43. Spin quantum number (ms)
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Excess oxygen
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Spin is +1/2 or -1/2 in an orbital

44. Resonance structures
Strong acids - strong bases - soluble salts
Same molecule - different electron pair positions
CO - produced from incomplete combustion - very toxic
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

45. Coal
OH - alcohols - name ends in ol
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Disordered systems with higher entropies are favored
Potassium - Calcium - Sodium

46. Sigma bonds
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
21% of atmosphere - colorless - odorless - supports combustion reactions
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
DH = bonds broken - bonds formed

47. London dispersion forces
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Mixture of copper and zinc
Classified as strong bases but not very soluble.
SO4²?

48. Isoelectronic
CO3²?
Two atoms with the same number of electrons
21% of atmosphere - colorless - odorless - supports combustion reactions
Yes in thermo - no in electro

49. Isotope
Solid at room temperature
4.184
Same element - different number of neutrons
Limited oxygen

50. Nitrate ion
It is at equilibrium
NO3?
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Degrade the oxone layer