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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. Color of MnO4? solution
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Gas pressure = atm pressure + height of mercury
Glass and plastic
Purple

2. Alkaline earth metals
Most stable
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
2nd group - fairly reactive - pastes are used in batteries
Gases at room temperature - used for fuel

3. Oxygen gas properties
21% of atmosphere - colorless - odorless - supports combustion reactions
2nd group - fairly reactive - pastes are used in batteries
NH2 - ends in -amide
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

4. Noble gases
Excess oxygen
SO4²?
Extremely slow reactivity
DH = bonds broken - bonds formed

5. Sigma bonds
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Mixture of copper - zinc - and other metals
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

6. Examples of strong electrolytes
Strong acids - strong bases - soluble salts
1st group - most reactive metal family - react violently with water - create basic solutions
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

7. Phenolphthalein: pH range and colors
8.3 to 10.0 - colorless to pink
Same formula - different structure
Same molecule - different electron pair positions
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

8. If G is positive - is the reaction spontaneous?
Decreased
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
No
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

9. When are gases MOST ideal?
Low pressures - high temperatures
Classified as strong bases but not very soluble.
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Gas pressure = atm pressure + height of mercury

10. Properties of acids
Increase right and up
Mixture of copper - zinc - and other metals
Red
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

11. Single Replacement / displacement reaction
More active element replaces less active element in a compound.
SO4²?
Gold
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.

12. Gibb's Free Energy equation
Solid at room temperature
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.
Orange
DG = DH - TDS

13. Octahedral
6 bonding - 90° - sp³d2² hybridization
More active element replaces less active element in a compound.
Insoluble
Excess oxygen

14. Carbon monoxide
Yellow to orange
4.5 to 8.3 - Red to blue
CO - produced from incomplete combustion - very toxic
2 bonding - 180° - sp hybridization

15. Rare earth elements
Periods 8 and 9 - lanthanides and actinides
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored
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

16. Azimuthal quantum number (l)
Liquid at room temperature - used to make gasoline and solvents
Defines shape of orbital
Oxide that reacts with water to form either an acid or a base
It is at equilibrium

17. Carbonate ion
Emission of electromagnetic energy after beta - positron - or alpha decay
CO3²?
2 bonding - 1 nonbonding
4.184

18. What is the equation used for heat transfer problems?
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
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Endothermic
Q = mcDT

19. Noble gas properties
Soluble except when containing alkaline earth metals
Photography
Most stable
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

20. Ionization energy
6.0 to 7.6 - yellow to blue
Black
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
Nonmetal oxides form acids - metal oxides form bases

21. Isotope
Glass and plastic
Most stable
Same element - different number of neutrons
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

22. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Glass and plastic
Gas pressure = atm pressure - height of mercury
Yes in thermo - no in electro
Most stable

23. Formula for calculating enthalpy change with bond energies
Increased
A compound breaks into two parts
COH functional group - name ends in -al
DH = bonds broken - bonds formed

24. Litmus: pH range and colors
4.5 to 8.3 - Red to blue
Two compound react to form two new compounds
Same molecule - different electron pair positions
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

25. How can hydrogen be produced?
NH4?
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
The solute is dissolved in the solvent.

26. Sulfide color: CuS - HgS - and PbS
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
More active element replaces less active element in a compound.
Black
Q = mcDT

27. London dispersion forces
COOH - ends in -oic acid
Properties of solutions that depend on the number of particles per solvent molecule
Yellow to orange
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

28. Phosphate ion
Lemon yellow
Black
PO4³?
Liquid at room temperature - used to make gasoline and solvents

29. Decomposition reaction
Excess oxygen
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
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.
A compound breaks into two parts

30. Magnetic quantum number (ml)
Strong acids - strong bases - soluble salts
Potassium - Calcium - Sodium
Orientation of orbital in space
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

31. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
Gas pressure = atm pressure + height of mercury
Soluble except when containing alkaline earth metals
Defines shape of orbital
Orientation of orbital in space

32. Charles' Law
Solid at room temperature
V1/T1 = V2/T2
Photography
Miscible with water - flammable - used as fuel - poisonous

33. Alkali Metals
Increases left and down
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Emission of electromagnetic energy after beta - positron - or alpha decay
1st group - most reactive metal family - react violently with water - create basic solutions

34. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
PO4³?
Pressure of mixture of gases equals some of individual gas pressures.
Miscible with water - flammable - used as fuel - poisonous

35. Oxides are insoluble and when reacted with water..
Nonmetal oxides form acids - metal oxides form bases
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Increases left and down
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

36. Carboxylic acid group
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Properties of solutions that depend on the number of particles per solvent molecule
COOH - ends in -oic acid

37. Combustion reaction
2 bonding - 1 nonbonding
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Mixture of copper - zinc - and other metals
Endothermic

38. What metal will react in hot water?
R-O-R functional group - shorter chain ends in oxy - other is ane
Electrons are free to move through metal structure - high conductivity - ductile
Magnesium
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

39. Carboxylic acid
COOH functional group - name ends in oic acid
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
8.3 to 10.0 - colorless to pink
Black

40. Colloid
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
Two atoms with the same number of electrons
C2H3O2?
Green

41. Define heat of fusion.
Decreased
Stronger
Magnesium
Heat required to make a substance melt.

42. Allotropic forms of carbon
Diamond - graphite - amorphous - fullerenes
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
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block

43. Molality
Moles of solute / kg solvent
4.184
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Disordered systems with higher entropies are favored

44. Atomic radius trend
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 negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Increases left and down
DG = DH - TDS

45. Synthesis reaction
Two reactants combine to form a single product
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
The solute is dissolved in the solvent.
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

46. Alkali metal properties
Increase right and up
Moles of solute / kg solvent
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Excess oxygen

47. General Properties of Organic Compounds
Orange
Orange
Mixture of tin - copper - bismuth - and antimony
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

48. What is the second law of thermodynamics?
Classified as strong bases but not very soluble.
Liquid at room temperature - used to make gasoline and solvents
Disordered systems with higher entropies are favored
Miscible with water - flammable - used as fuel - poisonous

49. Amine group
NH2 - ends in -amide
PO4³?
Deadly - yellow-green - weapon
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

50. Color of excited Li+ - Sr2+ - Ca2+
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
Red
4.5 to 8.3 - Red to blue
Nonmetal oxides form acids - metal oxides form bases