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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. Supersaturated solution
6 bonding - 90° - sp³d2² hybridization
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
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
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

2. Gamma decay
6.0 to 7.6 - yellow to blue
Purple
Degrade the oxone layer
Emission of electromagnetic energy after beta - positron - or alpha decay

3. Alkali metal compounds and NH4? compounds are...
Soluble
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Pressure of mixture of gases equals some of individual gas pressures.
DTb = (Kb)(msolute)(i) - for water Kb is 0.51

4. Trigonal pyramidal
3 bonding - 1 nonbonding 107°
Emission of electromagnetic energy after beta - positron - or alpha decay
Blue-green
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

5. Beta particle
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Increased
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
6 bonding - 90° - sp³d2² hybridization

6. Alpha particle
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Green
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
Energy level - as it increases electrons are less bound to the nucleus

7. Sulfide color: CuS - HgS - and PbS
Black
PO4³?
Liquid at room temperature - used to make gasoline and solvents
3 bonding - 120° - sp² hybridization

8. Sterling silver
Mixture of silver and copper
yellow
PO4³?
OH - alcohols - name ends in ol

9. Methanol
Excess oxygen
Miscible with water - flammable - used as fuel - poisonous
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
4 bonding - 109.5° - sp³ hybridization

10. Chlorofluorocarbons
Gold
Diamond - graphite - amorphous - fullerenes
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.
Degrade the oxone layer

11. Boiling point elevation formula
P1/V1 = P2/V2
Disordered systems with higher entropies are favored
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
Gases at room temperature - used for fuel

12. Ionization energy
P1/V1 = P2/V2
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Increase right and up
Nonmetal oxides form acids - metal oxides form bases

13. Hydrogen gas properties
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
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
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
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.

14. Color of Fe3+ solution
Yellow to orange
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
3.1 - 4.4 - red to yellow

15. Double replacement reaction
Two compound react to form two new compounds
Gas pressure = atm pressure - height of mercury
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Black

16. Bent
Low pressures - high temperatures
2 bonding - 1 nonbonding
DG = DH - TDS
A compound breaks into two parts

17. What is the second law of thermodynamics?
Disordered systems with higher entropies are favored
Gas pressure = atm pressure + height of mercury
Soluble
Black

18. Properties of bases
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

19. Covalent bond
Soluble
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.
Black
Light green

20. Formula for calculating enthalpy change with bond energies
2nd group - fairly reactive - pastes are used in batteries
PO4³?
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
DH = bonds broken - bonds formed

21. Sulfide color: Sb2S3
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Orange
Mixture of tin - copper - bismuth - and antimony

22. Chlorine gas
Defines shape of orbital
No two electrons can have the same set of 4 quantum numbers
Deadly - yellow-green - weapon
Same molecule - different electron pair positions

23. When a reaction is endothermic - the entropy is
NO3?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
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
Increased

24. Single Replacement / displacement reaction
More active element replaces less active element in a compound.
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Increased
CO3²?

25. Color of CrO4²? solution
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
7th group - form salts - always exist as diatomic molecules - used in modern lighting
4.5 to 8.3 - Red to blue
Yellow

26. Compounds with 5-10 carbons
yellow
V1/T1 = V2/T2
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Liquid at room temperature - used to make gasoline and solvents

27. Ionic bond
Oxide that reacts with water to form either an acid or a base
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Electrons are free to move through metal structure - high conductivity - ductile
6.0 to 7.6 - yellow to blue

28. General Properties of Organic Compounds
COOH - ends in -oic acid
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
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

29. Carboxylic acid group
Acid to water
COOH - ends in -oic acid
Mixture of silver and copper
Purple

30. Color of excited K+
2 bonding - 1 nonbonding
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Purple/pink
Defines shape of orbital

31. Oxygen gas properties
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
It is at equilibrium
21% of atmosphere - colorless - odorless - supports combustion reactions
Lemon yellow

32. amphoteric
Make up jet fuels and kerosene
Substance can act either as an acid or a base
Purple/pink
Same molecule - different electron pair positions

33. Isotope
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
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
More active element replaces less active element in a compound.
Same element - different number of neutrons

34. Ethanol
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Potassium - Calcium - Sodium
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

35. Rare earth elements
Periods 8 and 9 - lanthanides and actinides
Purple
Acid to water
OH - alcohols - name ends in ol

36. Incomplete combustion occurs when there is
Bright yellow
Energy level - as it increases electrons are less bound to the nucleus
Blue
Limited oxygen

37. Carbon monoxide
Light green
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
CO - produced from incomplete combustion - very toxic
Limited oxygen

38. Graham's Law
Mixture of copper - zinc - and other metals
yellow
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Soluble except when containing Ag? - Hg2²? - or Pb²?

39. Oxides are insoluble and when reacted with water..
Increases left and down
Energy level - as it increases electrons are less bound to the nucleus
Nonmetal oxides form acids - metal oxides form bases
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

40. Amine group
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Two compound react to form two new compounds
Mixture of silver and copper
NH2 - ends in -amide

41. If G is negative - is the reaction spontaneous?
Yes
Lemon yellow
R-O-R functional group - shorter chain ends in oxy - other is ane
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

42. Bromthymol blue: pH range and colors
6.0 to 7.6 - yellow to blue
Yellow to orange
Substance can act either as an acid or a base
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

43. Molality
Moles of solute / kg solvent
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Moles / L
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

44. Azimuthal quantum number (l)
P1/V1 = P2/V2
Defines shape of orbital
Pressure of mixture of gases equals some of individual gas pressures.
Mixture of copper - zinc - and other metals

45. Covalent-network / atomic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
2 bonding - 180° - sp hybridization
Same element - different number of neutrons
It is at equilibrium

46. Color of excited Ba2+
5 bonding - 90° and 120° - sp³d hybridization
R-O-R functional group - shorter chain ends in oxy - other is ane
Blue-green
Light green

47. Pauli exclusion principle
OH functional group - name ends in -ol
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
No two electrons can have the same set of 4 quantum numbers

48. Linear
yellow
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
2 bonding - 180° - sp hybridization

49. Trigonal planar
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Moles of solute / kg solvent
Mixture of tin - copper - bismuth - and antimony
3 bonding - 120° - sp² hybridization

50. How can hydrogen be produced?
SO4²?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Black
Q = mcDT