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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.
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. Sterling silver
Extremely slow reactivity
Mixture of silver and copper
4.5 to 8.3 - Red to blue
C2H3O2?

2. Isoelectronic
Glass and plastic
Miscible with water - flammable - used as fuel - poisonous
Two atoms with the same number of electrons
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

3. General properties of alloys
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
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Spin is +1/2 or -1/2 in an orbital

4. Methyl orange: pH range and colors
3.1 - 4.4 - red to yellow
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
More active element replaces less active element in a compound.
Two reactants combine to form a single product

5. Graham's Law
DG = DH - TDS
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

6. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
PO4³?
Strong acids - strong bases - soluble salts
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

7. Bromthymol blue: pH range and colors
Heat required to make a substance melt.
6.0 to 7.6 - yellow to blue
Gases at room temperature - used for fuel
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

8. Amine
A compound breaks into two parts
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
NH2 functional group - name ends in -amide

9. Color of Cu2+ solution
Insoluble
Pressure of mixture of gases equals some of individual gas pressures.
Blue
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

10. Gamma decay
Emission of electromagnetic energy after beta - positron - or alpha decay
Disordered systems with higher entropies are favored
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Insoluble

11. Bent
Glass and plastic
The solute is dissolved in the solvent.
2 bonding - 1 nonbonding
Purple

12. Hydrogen gas properties
3 bonding - 1 nonbonding 107°
Pressure of mixture of gases equals some of individual gas pressures.
Etching glass and frosting lightblubs
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

13. Coal
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Mixture of tin - copper - bismuth - and antimony
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

14. Steel
Light green
Mixture of iron and carbon
COOH functional group - name ends in oic acid
Purple/pink

15. Covalent bond
P1/V1 = P2/V2
Energy level - as it increases electrons are less bound to the nucleus
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.
OH functional group - name ends in -ol

16. Hydrolysis reaction
White
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
3 bonding - 120° - sp² hybridization
Involves water

17. If G is zero - what is happening in the reaction?
COH functional group - name ends in -al
It is at equilibrium
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Same formula - different structure

18. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
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
Deadly - yellow-green - weapon
OH functional group - name ends in -ol

19. Electron affinity
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
5 bonding - 90° and 120° - sp³d hybridization
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Light green

20. Chlorine gas
Deadly - yellow-green - weapon
Excess oxygen
Liquid at room temperature - used to make gasoline and solvents
Black

21. Colloid
7th group - form salts - always exist as diatomic molecules - used in modern lighting
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
Same element - different number of neutrons
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

22. Tetrahedral
4 bonding - 109.5° - sp³ hybridization
Nonmetal oxides form acids - metal oxides form bases
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
Deadly - yellow-green - weapon

23. Acetate ion
C2H3O2?
Increase right and up
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Soluble

24. Sulfide color: Sb2S3
Magnesium
Orange
Yes in thermo - no in electro
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

25. Dalton's Law
Pressure of mixture of gases equals some of individual gas pressures.
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
Limited oxygen
1st group - most reactive metal family - react violently with water - create basic solutions

26. Sulfide color: CuS - HgS - and PbS
Black
4.184
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
Etching glass and frosting lightblubs

27. What 3 metals will react with cold water?
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Electrons are free to move through metal structure - high conductivity - ductile
CO3²?
Potassium - Calcium - Sodium

28. Molality
Do not conduct electricity well
Moles of solute / kg solvent
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Insoluble

29. Nitrate ion
Energy level - as it increases electrons are less bound to the nucleus
Soluble
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
NO3?

30. Aldehydes
Nonmetal oxides form acids - metal oxides form bases
8.3 to 10.0 - colorless to pink
Increases left and down
COH functional group - name ends in -al

31. Halogens
7th group - form salts - always exist as diatomic molecules - used in modern lighting
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

32. pewter
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Increase right and up
Mixture of tin - copper - bismuth - and antimony

33. Freezing point depression formula
Etching glass and frosting lightblubs
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Blue

34. Color of Fe3+ solution
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Yellow to orange
Gas pressure = atm pressure + height of mercury
Degrade the oxone layer

35. Properties of molecular crystals and liquids

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36. What metal will react in hot water?
Magnesium
COOH - ends in -oic acid
Make up jet fuels and kerosene
8.3 to 10.0 - colorless to pink

37. Add acid to water or water to acid
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Magnesium
Acid to water

38. Boiling point elevation formula
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Photography
Purple

39. Dilution equation
M1V1 = M2V2
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Defines shape of orbital

40. Molecular solids
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Mixture of iron and carbon

41. Define heat of fusion.
Liquid at room temperature - used to make gasoline and solvents
Heat required to make a substance melt.
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Mixture of copper and zinc

42. Examples of strong electrolytes
COOH functional group - name ends in oic acid
Strong acids - strong bases - soluble salts
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

43. Carbonate ion
CO3²?
Soluble
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

44. Ionization energy
Blue-green
Q = mcDT
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

45. Color of excited K+
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Two reactants combine to form a single product
Purple/pink

46. What kind of bonds generally hold liquids together?
It is at equilibrium
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Covalent
Red

47. Compounds with 1-4 carbons
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Gases at room temperature - used for fuel

48. Phosphate ion
Purple
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Make up jet fuels and kerosene
PO4³?

49. What are the allotropic forms of sulfur?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
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
Spin is +1/2 or -1/2 in an orbital

50. What is the equation used for heat transfer problems?
No
NO3?
Q = mcDT
CO3²?