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SAT Subject Test: Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Define heat of fusion.
Same formula - different structure
8.3 to 10.0 - colorless to pink
Green
Heat required to make a substance melt.

2. Hydroxyl group
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Do not conduct electricity well
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
OH - alcohols - name ends in ol

3. Ethers
R-O-R functional group - shorter chain ends in oxy - other is ane
Soluble except when containing alkaline earth metals
NO3?
Excess oxygen

4. Color of Ni2+ solution
Acid to water
ClO3?
Covalent
Green

5. Complete combustion occurs when there is
Excess oxygen
NH4?
Q = mcDT
Involves water

6. Examples of strong electrolytes
7th group - form salts - always exist as diatomic molecules - used in modern lighting
SO4²?
Strong acids - strong bases - soluble salts
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

7. Magnetic quantum number (ml)
Orientation of orbital in space
Deadly - yellow-green - weapon
Yes in thermo - no in electro
Soluble except when containing alkaline earth metals

8. General Properties of Organic Compounds
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
3 bonding - 120° - sp² hybridization
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

9. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Properties of solutions that depend on the number of particles per solvent molecule
The solute is dissolved in the solvent.
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Gas pressure = atm pressure + height of mercury

10. Equation when using a barometer to calculate gas pressure.
Gas pressure = atm pressure - height of mercury
Orange
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

11. Alkali metal compounds and NH4? compounds are...
Soluble
Do not conduct electricity well
Orange
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

12. Single Replacement / displacement reaction
More active element replaces less active element in a compound.
Properties of solutions that depend on the number of particles per solvent molecule
R-O-R functional group - shorter chain ends in oxy - other is ane
Do not conduct electricity well

13. Color of excited Na+
M1V1 = M2V2
yellow
4.184
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

14. Resonance structures
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Miscible with water - flammable - used as fuel - poisonous
Gases at room temperature - used for fuel
Same molecule - different electron pair positions

15. Hydrogen gas properties
Miscible with water - flammable - used as fuel - poisonous
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Disordered systems with higher entropies are favored
Q = mcDT

16. List equivalent pressure values for mmHg - torr - atm - and Pa
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Involves water
No
Energy level - as it increases electrons are less bound to the nucleus

17. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Two compound react to form two new compounds
Soluble
Gases at room temperature - used for fuel

18. What qualifies as a strong base?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Same formula - different structure
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

19. Is removing an electron an exothermic or endothermic process?
Endothermic
Limited oxygen
COH functional group - name ends in -al
Yes in thermo - no in electro

20. Octahedral
Make up jet fuels and kerosene
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Bright yellow
6 bonding - 90° - sp³d2² hybridization

21. Examples of amorphous solids
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
Two atoms with the same number of electrons
Degrade the oxone layer
Glass and plastic

22. Rare earth elements
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
NO3?
Periods 8 and 9 - lanthanides and actinides
Covalent

23. Ester
Etching glass and frosting lightblubs
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Green

24. Supersaturated solution
Spin is +1/2 or -1/2 in an orbital
Q = mcDT
Soluble except when containing alkaline earth metals
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

25. Linear
2 bonding - 180° - sp hybridization
Gold
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
PO4³?

26. Boyle's Law
P1/V1 = P2/V2
Orientation of orbital in space
4.184
Mixture of tin - copper - bismuth - and antimony

27. Properties of molecular crystals and liquids

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28. Covalent-network / atomic solids
Insoluble
Acid to water
Black
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

29. Ketone
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Stronger
Orientation of orbital in space
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.

30. Solute vs. Solvent
The solute is dissolved in the solvent.
6.0 to 7.6 - yellow to blue
Heat required to make a substance melt.
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

31. Oxygen gas properties
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
21% of atmosphere - colorless - odorless - supports combustion reactions
Gases at room temperature - used for fuel
Gas pressure = atm pressure - height of mercury

32. How can hydrogen be produced?
Yes in thermo - no in electro
NH2 functional group - name ends in -amide
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
6 bonding - 90° - sp³d2² hybridization

33. Radioactivity
M1V1 = M2V2
Orange
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

34. Sulfide color: As2S3
Liquid at room temperature - used to make gasoline and solvents
Lemon yellow
Mixture of copper - zinc - and other metals
4.5 to 8.3 - Red to blue

35. Sulfide color: Sb2S3
Orange
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Same molecule - different electron pair positions
A compound breaks into two parts

36. What 3 metals will react with cold water?
Potassium - Calcium - Sodium
CO3²?
COOH - ends in -oic acid
Most stable

37. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Mixture of copper - zinc - and other metals
Oxide that reacts with water to form either an acid or a base

38. Molarity
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Acid to water
Soluble except when containing Ag? - Hg2²? - or Pb²?
Moles / L

39. Color of excited K+
Miscible with water - flammable - used as fuel - poisonous
Purple/pink
Glass and plastic
Gas pressure = atm pressure - height of mercury

40. Bromthymol blue: pH range and colors
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
6.0 to 7.6 - yellow to blue
Covalent
Liquid at room temperature - used to make gasoline and solvents

41. When a reaction is endothermic - the entropy is
Green
Increased
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Oxide that reacts with water to form either an acid or a base

42. Exceptions to the octet rule
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Emission of electromagnetic energy after beta - positron - or alpha decay
Decreased

43. What are the factors that affect reaction rate?
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Involves water
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

44. Double replacement reaction
Limited oxygen
PV = nRT - R = .0821
Two compound react to form two new compounds
Two reactants combine to form a single product

45. Carbonate ion
CO3²?
Mixture of copper - zinc - and other metals
Spin is +1/2 or -1/2 in an orbital
NO3?

46. Compounds with 18 carbons
Solid at room temperature
Increase right and up
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
NH2 - ends in -amide

47. Atomic radius trend
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Soluble except when containing Ag? - Hg2²? - or Pb²?
DH = bonds broken - bonds formed
Increases left and down

48. Transition metals
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Lemon yellow
3 bonding - 1 nonbonding 107°
SO4²?

49. Formula for calculating enthalpy change with bond energies
Limited oxygen
Two compound react to form two new compounds
DH = bonds broken - bonds formed
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

50. What are the allotropic forms of sulfur?
Blue
Glass and plastic
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

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SAT Subject Test: Chemistry

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