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SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. Suspension
Same formula - different structure
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
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
4.5 to 8.3 - Red to blue

2. Coal
Low pressures - high temperatures
Etching glass and frosting lightblubs
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Classified as strong bases but not very soluble.

3. Spin quantum number (ms)
yellow
Increase right and up
6 bonding - 90° - sp³d2² hybridization
Spin is +1/2 or -1/2 in an orbital

4. Nitrate ion
Yes
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
NO3?
Photography

5. What is the equation used for heat transfer problems?
Increases left and down
Two reactants combine to form a single product
Q = mcDT
NH2 - ends in -amide

6. Alchohols
COOH - ends in -oic acid
Limited oxygen
OH functional group - name ends in -ol
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

7. Bent
2 bonding - 1 nonbonding
Orientation of orbital in space
No
yellow

8. Silver bromide and silver iodide are used for
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Photography
Mixture of copper and zinc
Soluble except when containing alkaline earth metals

9. Alkali metal compounds and NH4? compounds are...
Soluble
1st group - most reactive metal family - react violently with water - create basic solutions
DG = DH - TDS
Orange

10. When the reaction is exothermic - the entropy is
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Emission of electromagnetic energy after beta - positron - or alpha decay
Increased
Decreased

11. Pi bonds
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.
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
4.184
DG = DH - TDS

12. Metallic solids
6.0 to 7.6 - yellow to blue
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
yellow

13. Dalton's Law
Pressure of mixture of gases equals some of individual gas pressures.
Potassium - Calcium - Sodium
Make up jet fuels and kerosene
CO3²?

14. Color of excited Ba2+
Blue
V1/T1 = V2/T2
Decreased
Light green

15. If G is positive - is the reaction spontaneous?
Gold
No
No two electrons can have the same set of 4 quantum numbers
Moles / L

16. 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
21% of atmosphere - colorless - odorless - supports combustion reactions
3 bonding - 120° - sp² hybridization
Magnesium

17. amphoteric
4.184
Substance can act either as an acid or a base
2 bonding - 1 nonbonding
Same molecule - different electron pair positions

18. If G is zero - what is happening in the reaction?
Mixture of tin - copper - bismuth - and antimony
It is at equilibrium
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

19. If G is negative - is the reaction spontaneous?
Yes
Periods 8 and 9 - lanthanides and actinides
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
1st group - most reactive metal family - react violently with water - create basic solutions

20. Alkali Metals
Limited oxygen
1st group - most reactive metal family - react violently with water - create basic solutions
Two atoms with the same number of electrons
Red

21. What is the second law of thermodynamics?
Photography
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Mixture of silver and copper
Disordered systems with higher entropies are favored

22. Phenolphthalein: pH range and colors
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
V1/T1 = V2/T2
Limited oxygen
8.3 to 10.0 - colorless to pink

23. Acetate ion
Make up jet fuels and kerosene
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
C2H3O2?
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

24. Color of excited K+
ClO3?
Purple/pink
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Miscible with water - flammable - used as fuel - poisonous

25. Litmus: pH range and colors
Green
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Covalent
4.5 to 8.3 - Red to blue

26. Covalent-network / atomic solids
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
White
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

27. What are the allotropic forms of sulfur?
Diamond - graphite - amorphous - fullerenes
The solute is dissolved in the solvent.
COOH - ends in -oic acid
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

28. Oxygen gas properties
Potassium - Calcium - Sodium
21% of atmosphere - colorless - odorless - supports combustion reactions
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
2nd group - fairly reactive - pastes are used in batteries

29. Chlorofluorocarbons
Oxide that reacts with water to form either an acid or a base
Degrade the oxone layer
Gas pressure = atm pressure - height of mercury
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

30. Oxides are insoluble and when reacted with water..
Nonmetal oxides form acids - metal oxides form bases
2nd group - fairly reactive - pastes are used in batteries
Gold
Insoluble

31. Principal quantum number (n)
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Gas pressure = atm pressure - height of mercury
Energy level - as it increases electrons are less bound to the nucleus
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

32. What are the factors that affect reaction rate?
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 iron and carbon
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Miscible with water - flammable - used as fuel - poisonous

33. Alkaline metal oxides are...
Yellow to orange
R-O-R functional group - shorter chain ends in oxy - other is ane
6 bonding - 90° - sp³d2² hybridization
Classified as strong bases but not very soluble.

34. Alkaline earth metals
DH = bonds broken - bonds formed
Photography
Limited oxygen
2nd group - fairly reactive - pastes are used in batteries

35. Carboxylic acid group
Spin is +1/2 or -1/2 in an orbital
COOH - ends in -oic acid
NH2 - ends in -amide
Increased

36. Cl - Br - and I compounds are...
More active element replaces less active element in a compound.
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 Ag? - Hg2²? - or Pb²?
Mixture of silver and copper

37. General Properties of Organic Compounds
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Diamond - graphite - amorphous - fullerenes
The solute is dissolved in the solvent.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

38. Ethanol
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
NH4?
Nonmetal oxides form acids - metal oxides form bases
Covalent

39. What qualifies as a strong base?
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Orientation of orbital in space
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

40. Properties of molecular crystals and liquids

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41. Ester
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Properties of solutions that depend on the number of particles per solvent molecule
Moles / L

42. Tetrahedral
V1/T1 = V2/T2
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
4 bonding - 109.5° - sp³ hybridization
PO4³?

43. Examples of amorphous solids
Yellow to orange
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Glass and plastic
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

44. Covalent bond
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
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.
C2H3O2?
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

45. SO4²? compounds are...
Liquid at room temperature - used to make gasoline and solvents
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

46. What metal will react in hot water?
Magnesium
Do not conduct electricity well
OH functional group - name ends in -ol
SO4²?

47. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Orientation of orbital in space
Lemon yellow
Moles of solute / kg solvent

48. Chlorine gas
The solute is dissolved in the solvent.
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Deadly - yellow-green - weapon

49. Decomposition reaction
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
A compound breaks into two parts
Mixture of copper and zinc
V1/T1 = V2/T2

50. When a reaction is endothermic - the entropy is
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Spin is +1/2 or -1/2 in an orbital
Increased
Heat required to make a substance melt.