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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. Examples of strong electrolytes
Soluble except when containing Ag? - Hg2²? - or Pb²?
Strong acids - strong bases - soluble salts
Magnesium
Purple/pink

2. Pauli exclusion principle
No two electrons can have the same set of 4 quantum numbers
PO4³?
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

3. Principal quantum number (n)
Soluble except when containing Ag? - Hg2²? - or Pb²?
Moles / L
Energy level - as it increases electrons are less bound to the nucleus
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

4. Color of Ni2+ solution
Potassium - Calcium - Sodium
Solid at room temperature
Green
Lemon yellow

5. Properties of ionic substances

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6. Allotropic forms of carbon
Liquid at room temperature - used to make gasoline and solvents
Mixture of iron and carbon
Diamond - graphite - amorphous - fullerenes
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

7. Sulfide color: CuS - HgS - and PbS
Yellow to orange
Black
Stronger
Gases at room temperature - used for fuel

8. What metal will react in hot water?
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Magnesium
Pressure of mixture of gases equals some of individual gas pressures.
PV = nRT - R = .0821

9. Compounds with 1-4 carbons
Defines shape of orbital
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Gases at room temperature - used for fuel
3 bonding - 1 nonbonding 107°

10. Gibb's Free Energy equation
DG = DH - TDS
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Involves water
Mixture of copper - zinc - and other metals

11. Acetate ion
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
C2H3O2?
DG = DH - TDS
OH - alcohols - name ends in ol

12. Aldehydes
2nd group - fairly reactive - pastes are used in batteries
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Liquid at room temperature - used to make gasoline and solvents
COH functional group - name ends in -al

13. Hydrofluoric acid is used for
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Substance can act either as an acid or a base
Two compound react to form two new compounds
Etching glass and frosting lightblubs

14. Equation when using a barometer to calculate gas pressure.
Gas pressure = atm pressure - height of mercury
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
Properties of solutions that depend on the number of particles per solvent molecule

15. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
A compound breaks into two parts
Covalent
Yellow to orange
Gas pressure = atm pressure + height of mercury

16. What is the second law of thermodynamics?
Increased
Deadly - yellow-green - weapon
Orientation of orbital in space
Disordered systems with higher entropies are favored

17. Properties of acids
Purple
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
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Mixture of copper - zinc - and other metals

18. Define heat of fusion.
Heat required to make a substance melt.
Periods 8 and 9 - lanthanides and actinides
Covalent
P1/V1 = P2/V2

19. List equivalent pressure values for mmHg - torr - atm - and Pa
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Periods 8 and 9 - lanthanides and actinides
4 bonding - 109.5° - sp³ hybridization
Nonmetal oxides form acids - metal oxides form bases

20. Carbonate ion
4.184
CO3²?
Mixture of iron and carbon
M1V1 = M2V2

21. Fusion
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Strong acids - strong bases - soluble salts
Classified as strong bases but not very soluble.

22. Hydroxyl group
OH - alcohols - name ends in ol
Limited oxygen
Two atoms with the same number of electrons
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

23. Properties of molecular crystals and liquids

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24. Sulfide color: Sb2S3
Spin is +1/2 or -1/2 in an orbital
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Orange
Moles of solute / kg solvent

25. Molecular solids
Energy level - as it increases electrons are less bound to the nucleus
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
8.3 to 10.0 - colorless to pink
Covalent

26. Covalent-network / atomic solids
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
5 bonding - 90° and 120° - sp³d hybridization
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

27. Dilution equation
Liquid at room temperature - used to make gasoline and solvents
NH2 functional group - name ends in -amide
M1V1 = M2V2
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

28. Amine
6.0 to 7.6 - yellow to blue
Photography
NH2 functional group - name ends in -amide
DG = DH - TDS

29. Chlorofluorocarbons
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Degrade the oxone layer
Do not conduct electricity well
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

30. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
Lemon yellow
Increased
Gas pressure = atm pressure - height of mercury

31. Boyle's Law
Increase right and up
Soluble except when containing alkaline earth metals
P1/V1 = P2/V2
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.

32. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Spin is +1/2 or -1/2 in an orbital
A compound breaks into two parts
Nonmetal oxides form acids - metal oxides form bases

33. Oxygen gas properties
5 bonding - 90° and 120° - sp³d hybridization
21% of atmosphere - colorless - odorless - supports combustion reactions
P1/V1 = P2/V2
No two electrons can have the same set of 4 quantum numbers

34. Name the six strong acids
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Potassium - Calcium - Sodium
Orange

35. Amine group
3 bonding - 120° - sp² hybridization
Green
Emission of electromagnetic energy after beta - positron - or alpha decay
NH2 - ends in -amide

36. Methyl orange: pH range and colors
Gas pressure = atm pressure - height of mercury
3.1 - 4.4 - red to yellow
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
NH2 functional group - name ends in -amide

37. Color of excited K+
1st group - most reactive metal family - react violently with water - create basic solutions
NH2 - ends in -amide
Purple/pink
Same molecule - different electron pair positions

38. Ionization energy
Two compound react to form two new compounds
COOH functional group - name ends in oic acid
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

39. Pi bonds
Spin is +1/2 or -1/2 in an orbital
Bright yellow
Most stable
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

40. Noble gases
Excess oxygen
Light green
Extremely slow reactivity
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

41. Boiling point elevation formula
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
NH2 - ends in -amide
NH2 functional group - name ends in -amide
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

42. Beta particle
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
NO3?
Soluble except when containing Ag? - Hg2²? - or Pb²?
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

43. amphoteric
Oxide that reacts with water to form either an acid or a base
Substance can act either as an acid or a base
Moles of solute / kg solvent
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

44. What is the ideal gas law?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
NH2 - ends in -amide
PV = nRT - R = .0821
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

45. Molarity
Deadly - yellow-green - weapon
Moles / L
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
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

46. Fission
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Increased
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

47. Metallic solids
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
OH - alcohols - name ends in ol
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Same molecule - different electron pair positions

48. Azimuthal quantum number (l)
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Defines shape of orbital
2 bonding - 180° - sp hybridization

49. Trigonal pyramidal
3 bonding - 1 nonbonding 107°
PO4³?
No
6.0 to 7.6 - yellow to blue

50. Color of CrO4²? solution
OH - alcohols - name ends in ol
Yellow
Soluble except when containing alkaline earth metals
Mixture of tin - copper - bismuth - and antimony