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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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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. General properties of alloys
Orientation of orbital in space
Mixture of silver and copper
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
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

2. If G is zero - what is happening in the reaction?
Orange
Degrade the oxone layer
Pressure of mixture of gases equals some of individual gas pressures.
It is at equilibrium

3. Isoelectronic
Two atoms with the same number of electrons
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
PV = nRT - R = .0821
Gases at room temperature - used for fuel

4. What kind of bonds generally hold liquids together?
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
R-O-R functional group - shorter chain ends in oxy - other is ane
Soluble except when containing Ag? - Hg2²? - or Pb²?
Covalent

5. Alkali Metals
C2H3O2?
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Same element - different number of neutrons
1st group - most reactive metal family - react violently with water - create basic solutions

6. Acetate ion
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
OH - alcohols - name ends in ol
C2H3O2?
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

7. Transition metals
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
Spin is +1/2 or -1/2 in an orbital
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

8. Suspension
3 bonding - 120° - sp² hybridization
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Green

9. Compounds with 18 carbons
Photography
PO4³?
2 bonding - 180° - sp hybridization
Solid at room temperature

10. What are the allotropic forms of sulfur?
No
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Moles of solute / kg solvent
4.184

11. Trigonal bipyramidal
Soluble
5 bonding - 90° and 120° - sp³d hybridization
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Yes in thermo - no in electro

12. If G is positive - is the reaction spontaneous?
White
2 bonding - 180° - sp hybridization
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
No

13. Supersaturated solution
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Excess oxygen
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Gases at room temperature - used for fuel

14. Colloid
Light green
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
Black
Strong acids - strong bases - soluble salts

15. Aldehydes
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Excess oxygen
COH functional group - name ends in -al
Heat required to make a substance melt.

16. Freezing point depression formula
Blue-green
4 bonding - 109.5° - sp³ hybridization
Bright yellow
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

17. Hydrolysis reaction
Involves water
Soluble
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Spin is +1/2 or -1/2 in an orbital

18. Color of excited Na+
Substance can act either as an acid or a base
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Soluble except when containing Ag? - Hg2²? - or Pb²?
yellow

19. Covalent bond
2 bonding - 180° - sp hybridization
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.
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

20. Ionization energy
Bright yellow
Covalent
SO4²?
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

21. If G is negative - is the reaction spontaneous?
Yes
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
PV = nRT - R = .0821
Same molecule - different electron pair positions

22. Chlorofluorocarbons
Degrade the oxone layer
3.1 - 4.4 - red to yellow
Increased
Do not conduct electricity well

23. Ester
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
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
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Soluble except when containing Ag? - Hg2²? - or Pb²?

24. Anhydride
Oxide that reacts with water to form either an acid or a base
8.3 to 10.0 - colorless to pink
Properties of solutions that depend on the number of particles per solvent molecule
Black

25. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Yellow to orange
Involves water
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

26. Color of excited Cu2+
Blue-green
Diamond - graphite - amorphous - fullerenes
SO4²?
OH - alcohols - name ends in ol

27. Magnetic quantum number (ml)
Orientation of orbital in space
Soluble except when containing alkaline earth metals
Red
Periods 8 and 9 - lanthanides and actinides

28. Molality
Moles of solute / kg solvent
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2
Involves water
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

29. When a reaction is endothermic - the entropy is
Make up jet fuels and kerosene
Soluble
Increased
Moles of solute / kg solvent

30. Sulfide color: Sb2S3
Emission of electromagnetic energy after beta - positron - or alpha decay
Two atoms with the same number of electrons
White
Orange

31. Cl - Br - and I compounds are...
6 bonding - 90° - sp³d2² hybridization
Soluble except when containing Ag? - Hg2²? - or Pb²?
2 bonding - 1 nonbonding
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

32. Halogen properties
Heat required to make a substance melt.
No
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Light green

33. What is the second law of thermodynamics?
Mixture of iron and carbon
Photography
Mixture of copper - zinc - and other metals
Disordered systems with higher entropies are favored

34. amphoteric
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
OH functional group - name ends in -ol
Substance can act either as an acid or a base
White

35. Color of Cu2+ solution
Increase right and up
Blue
Two reactants combine to form a single product
Orange

36. Carboxylic acid group
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
OH functional group - name ends in -ol
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
COOH - ends in -oic acid

37. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
Two atoms with the same number of electrons
6 bonding - 90° - sp³d2² hybridization
Liquid at room temperature - used to make gasoline and solvents

38. Gibb's Free Energy equation
DG = DH - TDS
Black
Same formula - different structure
Photography

39. What qualifies as a strong base?
3 bonding - 120° - sp² hybridization
The solute is dissolved in the solvent.
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Photography

40. Gamma decay
Deadly - yellow-green - weapon
Soluble
Emission of electromagnetic energy after beta - positron - or alpha decay
Same formula - different structure

41. Atomic radius trend
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Blue-green
Increases left and down
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

42. Pi bonds
Gas pressure = atm pressure - height of mercury
Substance can act either as an acid or a base
NO3?
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first

43. Hydroxyl group
Soluble
OH - alcohols - name ends in ol
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

44. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Soluble
Gas pressure = atm pressure - height of mercury
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Yes in thermo - no in electro

45. How can hydrogen be produced?
OH functional group - name ends in -ol
Insoluble
7th group - form salts - always exist as diatomic molecules - used in modern lighting
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

46. Synthesis reaction
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
More active element replaces less active element in a compound.
Two reactants combine to form a single product
Same element - different number of neutrons

47. Steel
8.3 to 10.0 - colorless to pink
Do not conduct electricity well
Soluble
Mixture of iron and carbon

48. Alpha particle
5 bonding - 90° and 120° - sp³d hybridization
21% of atmosphere - colorless - odorless - supports combustion reactions
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
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

49. Trigonal planar
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
3 bonding - 120° - sp² hybridization

50. Sulfide color: CdS
Defines shape of orbital
Bright yellow
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
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1