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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
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Spin is +1/2 or -1/2 in an orbital
Strong acids - strong bases - soluble salts

2. Ammonium Ion
Bright yellow
NH4?
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
NH2 functional group - name ends in -amide

3. Ketone
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Mixture of copper and zinc
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Covalent

4. Alkali Metals
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Extremely slow reactivity
1st group - most reactive metal family - react violently with water - create basic solutions

5. Silver bromide and silver iodide are used for
NO3?
Photography
Pressure of mixture of gases equals some of individual gas pressures.
yellow

6. bronze
Mixture of copper - zinc - and other metals
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

7. Isomer
Same formula - different structure
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Two compound react to form two new compounds

8. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Yes in thermo - no in electro
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Excess oxygen

9. Ethers
R-O-R functional group - shorter chain ends in oxy - other is ane
Light green
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

10. Allotropic forms of carbon
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Diamond - graphite - amorphous - fullerenes
ClO3?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

11. What are the factors that affect reaction rate?
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Defines shape of orbital
SO4²?

12. Properties of bases
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Increases left and down
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

13. Steel
Light green
Mixture of iron and carbon
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
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components

14. Compounds with 5-10 carbons
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Stronger
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Liquid at room temperature - used to make gasoline and solvents

15. Exceptions to the octet rule
Covalent
1st group - most reactive metal family - react violently with water - create basic solutions
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

16. Principal quantum number (n)
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Energy level - as it increases electrons are less bound to the nucleus
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
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.

17. Sulfide color: CuS - HgS - and PbS
PV = nRT - R = .0821
It is at equilibrium
NH2 functional group - name ends in -amide
Black

18. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Soluble
Purple
Lemon yellow

19. Linear
2 bonding - 180° - sp hybridization
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Spin is +1/2 or -1/2 in an orbital

20. What are the allotropic forms of sulfur?
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
CO3²?
Limited oxygen

21. Ionization energy
White
No
SO4²?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

22. Is removing an electron an exothermic or endothermic process?
Endothermic
Excess oxygen
PO4³?
Oxide that reacts with water to form either an acid or a base

23. Properties of molecular crystals and liquids

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24. Coal
Electrons are free to move through metal structure - high conductivity - ductile
P1/V1 = P2/V2
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Soluble

25. Acetate ion
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
5 bonding - 90° and 120° - sp³d hybridization
C2H3O2?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

26. If G is zero - what is happening in the reaction?
It is at equilibrium
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Acid to water
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A

27. Trigonal pyramidal
NO3?
Yellow
3 bonding - 1 nonbonding 107°
A compound breaks into two parts

28. Ester
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
COH functional group - name ends in -al
Stronger

29. Properties of acids
Two atoms with the same number of electrons
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
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
Soluble except when containing alkaline earth metals

30. Molality
Defines shape of orbital
Light green
Moles of solute / kg solvent
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

31. Noble gases
Q = mcDT
Extremely slow reactivity
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
White

32. Freezing point depression formula
Stronger
Limited oxygen
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Acid to water

33. Octahedral
Same molecule - different electron pair positions
6 bonding - 90° - sp³d2² hybridization
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Degrade the oxone layer

34. Sulfide color: As2S3
Increase right and up
Two atoms with the same number of electrons
Lemon yellow
Orientation of orbital in space

35. What qualifies as a strong base?
6.0 to 7.6 - yellow to blue
Oxide that reacts with water to form either an acid or a base
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?

36. Nonmetals
PV = nRT - R = .0821
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Do not conduct electricity well
Miscible with water - flammable - used as fuel - poisonous

37. Gibb's Free Energy equation
DG = DH - TDS
Purple/pink
Two compound react to form two new compounds
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

38. Decomposition reaction
Electrons are free to move through metal structure - high conductivity - ductile
Potassium - Calcium - Sodium
A compound breaks into two parts
Light green

39. Isoelectronic
Pressure of mixture of gases equals some of individual gas pressures.
Two atoms with the same number of electrons
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Potassium - Calcium - Sodium

40. Molarity
No
Moles / L
2nd group - fairly reactive - pastes are used in batteries
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

41. Magnetic quantum number (ml)
Defines shape of orbital
Orientation of orbital in space
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Mixture of silver and copper

42. Compounds with 12-18 carbons
Increases left and down
Gas pressure = atm pressure - height of mercury
Make up jet fuels and kerosene
PV = nRT - R = .0821

43. Complete combustion occurs when there is
Excess oxygen
3 bonding - 120° - sp² hybridization
Covalent
P1/V1 = P2/V2

44. General Properties of Organic Compounds
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Bright yellow
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

45. Incomplete combustion occurs when there is
Excess oxygen
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Limited oxygen

46. Petroleum
SO4²?
4 bonding - 109.5° - sp³ hybridization
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Periods 8 and 9 - lanthanides and actinides

47. Sigma bonds
6 bonding - 90° - sp³d2² hybridization
Classified as strong bases but not very soluble.
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
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

48. Amine
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
The solute is dissolved in the solvent.
Deadly - yellow-green - weapon
NH2 functional group - name ends in -amide

49. Hydrolysis reaction
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Involves water
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

50. Solute vs. Solvent
Mixture of silver and copper
The solute is dissolved in the solvent.
SO4²?
1st group - most reactive metal family - react violently with water - create basic solutions