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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. How many joules are in a calorie?
4.184
DH = bonds broken - bonds formed
Most stable
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred

2. Ammonium Ion
Soluble except when containing Ag? - Hg2²? - or Pb²?
NH4?
Increase right and up
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

3. Gibb's Free Energy equation
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Two reactants combine to form a single product
Soluble
DG = DH - TDS

4. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Gas pressure = atm pressure + height of mercury
Purple/pink

5. Dipole-dipole forces (including hydrogen 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.
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
2 bonding - 1 nonbonding

6. Aldehydes
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
COH functional group - name ends in -al
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
Endothermic

7. Color of excited Li+ - Sr2+ - Ca2+
Gold
Gas pressure = atm pressure - height of mercury
Red
Blue

8. Alkali metal properties
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
It is at equilibrium
Yellow to orange
Limited oxygen

9. General Properties of Organic Compounds
Mixture of silver and copper
Involves water
Same molecule - different electron pair positions
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

10. Electron affinity
3.1 - 4.4 - red to yellow
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Classified as strong bases but not very soluble.
Limited oxygen

11. Chlorate ion
COOH functional group - name ends in oic acid
Yes
Increase right and up
ClO3?

12. Trigonal planar
3 bonding - 120° - sp² hybridization
COOH - ends in -oic acid
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Moles / L

13. Compounds with 12-18 carbons
Make up jet fuels and kerosene
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.
COOH - ends in -oic acid
Involves water

14. Nitrate ion
4.5 to 8.3 - Red to blue
Moles of solute / kg solvent
4 bonding - 109.5° - sp³ hybridization
NO3?

15. Sulfate ion
Mixture of silver and copper
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
SO4²?
R-O-R functional group - shorter chain ends in oxy - other is ane

16. Equation when using a barometer to calculate gas pressure.
Make up jet fuels and kerosene
Bright yellow
Heat required to make a substance melt.
Gas pressure = atm pressure - height of mercury

17. amphoteric
Gas pressure = atm pressure + height of mercury
Substance can act either as an acid or a base
Etching glass and frosting lightblubs
C2H3O2?

18. Pauli exclusion principle
Same molecule - different electron pair positions
Same formula - different structure
Spin is +1/2 or -1/2 in an orbital
No two electrons can have the same set of 4 quantum numbers

19. Litmus: pH range and colors
2 bonding - 1 nonbonding
5 bonding - 90° and 120° - sp³d hybridization
4.5 to 8.3 - Red to blue
NH2 functional group - name ends in -amide

20. Colloid
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Covalent
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
Properties of solutions that depend on the number of particles per solvent molecule

21. Alchohols
OH functional group - name ends in -ol
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Mixture of copper and zinc
Heat required to make a substance melt.

22. Exceptions to the octet rule
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
4.5 to 8.3 - Red to blue
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Degrade the oxone layer

23. Sulfide color: CuS - HgS - and PbS
Black
Excess oxygen
NH2 - ends in -amide
Light green

24. Resonance structures
PO4³?
Purple
Glass and plastic
Same molecule - different electron pair positions

25. Octahedral
6 bonding - 90° - sp³d2² hybridization
SO4²?
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Miscible with water - flammable - used as fuel - poisonous

26. Beta particle
Oxide that reacts with water to form either an acid or a base
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Yes in thermo - no in electro
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

27. Alpha particle
2 bonding - 1 nonbonding
Nonmetal oxides form acids - metal oxides form bases
5 bonding - 90° and 120° - sp³d hybridization
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

28. Phenolphthalein: pH range and colors
8.3 to 10.0 - colorless to pink
Energy level - as it increases electrons are less bound to the nucleus
Mixture of silver and copper
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

29. Isotope
Same element - different number of neutrons
Deadly - yellow-green - weapon
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Yellow

30. Spin quantum number (ms)
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
COH functional group - name ends in -al
Spin is +1/2 or -1/2 in an orbital
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

31. Dalton's Law
Mixture of iron and carbon
Mixture of copper - zinc - and other metals
Two reactants combine to form a single product
Pressure of mixture of gases equals some of individual gas pressures.

32. Chlorofluorocarbons
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Stronger
A compound breaks into two parts
Degrade the oxone layer

33. Color of excited Cu2+
4.184
Blue-green
Orange
Mixture of tin - copper - bismuth - and antimony

34. Rare earth elements
Magnesium
Periods 8 and 9 - lanthanides and actinides
8.3 to 10.0 - colorless to pink
P1/V1 = P2/V2

35. Color of excited Na+
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
CO3²?
yellow
Properties of solutions that depend on the number of particles per solvent molecule

36. Carbonate ion
Blue-green
A compound breaks into two parts
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
CO3²?

37. Pi bonds
21% of atmosphere - colorless - odorless - supports combustion reactions
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
No two electrons can have the same set of 4 quantum numbers
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates

38. When a reaction is endothermic - the entropy is
Increased
Green
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.
Lemon yellow

39. Examples of amorphous solids
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
4 bonding - 109.5° - sp³ hybridization
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
Glass and plastic

40. Supersaturated solution
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
3.1 - 4.4 - red to yellow
Strong acids - strong bases - soluble salts
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

41. Colligative properties
Mixture of silver and copper
V1/T1 = V2/T2
Endothermic
Properties of solutions that depend on the number of particles per solvent molecule

42. Boyle's Law
Same element - different number of neutrons
Do not conduct electricity well
21% of atmosphere - colorless - odorless - supports combustion reactions
P1/V1 = P2/V2

43. Sulfide color: Sb2S3
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
C2H3O2?
Orange
Energy level - as it increases electrons are less bound to the nucleus

44. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Yes in thermo - no in electro
2 bonding - 1 nonbonding
Solid at room temperature
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

45. Allotropic forms of carbon
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Diamond - graphite - amorphous - fullerenes
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Lemon yellow

46. Sulfide color: CdS
Bright yellow
Yes
CO - produced from incomplete combustion - very toxic
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

47. Tetrahedral
3 bonding - 1 nonbonding 107°
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
4 bonding - 109.5° - sp³ hybridization
Defines shape of orbital

48. Oxides are insoluble and when reacted with water..
Limited oxygen
Covalent
Nonmetal oxides form acids - metal oxides form bases
Stronger

49. Incomplete combustion occurs when there is
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Limited oxygen
Magnesium
NO3?

50. Acids with more oxygen atoms are
Stronger
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
Black