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SAT Subject Test: Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Formula for calculating enthalpy change with bond energies
Same formula - different structure
DH = bonds broken - bonds formed
Liquid at room temperature - used to make gasoline and solvents
Mixture of copper - zinc - and other metals

2. Chlorine gas
Gold
3 bonding - 120° - sp² hybridization
Deadly - yellow-green - weapon
4 bonding - 109.5° - sp³ hybridization

3. Equation when using a barometer to calculate gas pressure.
COOH functional group - name ends in oic acid
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Gas pressure = atm pressure - height of mercury
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent

4. Dilution equation
M1V1 = M2V2
3.1 - 4.4 - red to yellow
Yellow
Purple

5. General Properties of Organic Compounds
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Mixture of tin - copper - bismuth - and antimony
DH = bonds broken - bonds formed
NH2 functional group - name ends in -amide

6. Methyl orange: pH range and colors
6.0 to 7.6 - yellow to blue
3.1 - 4.4 - red to yellow
Miscible with water - flammable - used as fuel - poisonous
Pressure of mixture of gases equals some of individual gas pressures.

7. Do you multiply by coefficients in thermochemistry problems and electrochemistry problems?
Bright yellow
Yes in thermo - no in electro
yellow
Gases at room temperature - used for fuel

8. Phenolphthalein: pH range and colors
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
8.3 to 10.0 - colorless to pink

9. Graham's Law
Increases left and down
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
3 bonding - 1 nonbonding 107°
NH4?

10. Carbonate ion
CO3²?
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
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
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

11. Methanol
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Miscible with water - flammable - used as fuel - poisonous
Degrade the oxone layer

12. Beta particle
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
NO3?
Strong acids - strong bases - soluble salts
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

13. Ethers
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Defines shape of orbital
2nd group - fairly reactive - pastes are used in batteries
R-O-R functional group - shorter chain ends in oxy - other is ane

14. London dispersion forces
Involves water
V1/T1 = V2/T2
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Same molecule - different electron pair positions

15. Fission
Defines shape of orbital
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

16. Hydroxyl group
OH - alcohols - name ends in ol
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
The solute is dissolved in the solvent.
Red

17. What is the equation used for heat transfer problems?
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Q = mcDT
Disordered systems with higher entropies are favored
Light green

18. Color of excited Na+
Increased
Moles / L
Energy level - as it increases electrons are less bound to the nucleus
yellow

19. Oxides are insoluble and when reacted with water..
Nonmetal oxides form acids - metal oxides form bases
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
SO4²?
NH2 functional group - name ends in -amide

20. Carbon dioxide gas properties
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
3 bonding - 1 nonbonding 107°
Endothermic
Low pressures - high temperatures

21. Resonance structures
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Periods 8 and 9 - lanthanides and actinides
ClO3?
Same molecule - different electron pair positions

22. Sulfide color: Sb2S3
5 bonding - 90° and 120° - sp³d hybridization
Diamond - graphite - amorphous - fullerenes
6 bonding - 90° - sp³d2² hybridization
Orange

23. Properties of bases
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
Mixture of iron and carbon
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Blue

24. Tetrahedral
4 bonding - 109.5° - sp³ hybridization
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Nonmetal oxides form acids - metal oxides form bases
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

25. Ketone
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Increased
8.3 to 10.0 - colorless to pink
21% of atmosphere - colorless - odorless - supports combustion reactions

26. Covalent bond
Yellow
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 metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

27. Add acid to water or water to acid
Do not conduct electricity well
Pressure of mixture of gases equals some of individual gas pressures.
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Acid to water

28. Noble gases
2 bonding - 180° - sp hybridization
Extremely slow reactivity
Defines shape of orbital
COH functional group - name ends in -al

29. Trigonal pyramidal
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Same formula - different structure
3 bonding - 1 nonbonding 107°

30. Principal quantum number (n)
Orientation of orbital in space
Same element - different number of neutrons
CO3²?
Energy level - as it increases electrons are less bound to the nucleus

31. What are the allotropic forms of sulfur?
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
Do not conduct electricity well
DG = DH - TDS
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

32. Octahedral
CO3²?
Mixture of copper and zinc
6 bonding - 90° - sp³d2² hybridization
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

33. Molarity
Moles / L
Properties of solutions that depend on the number of particles per solvent molecule
Yes in thermo - no in electro
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

34. Properties of acids
Acid to water
Degrade the oxone layer
Oxide that reacts with water to form either an acid or a base
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

35. SO4²? compounds are...
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
21% of atmosphere - colorless - odorless - supports combustion reactions

36. Sulfate ion
3 bonding - 120° - sp² 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
SO4²?
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

37. Single Replacement / displacement reaction
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Green
R-O-R functional group - shorter chain ends in oxy - other is ane
More active element replaces less active element in a compound.

38. Solute vs. Solvent
The solute is dissolved in the solvent.
Orange
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

39. Alkali metal properties
OH - alcohols - name ends in ol
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
4.184

40. Halogen properties
2nd group - fairly reactive - pastes are used in batteries
Degrade the oxone layer
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
A compound breaks into two parts

41. Compounds with 5-10 carbons
Liquid at room temperature - used to make gasoline and solvents
Same molecule - different electron pair positions
2nd group - fairly reactive - pastes are used in batteries
The solute is dissolved in the solvent.

42. Carboxylic acid
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
COOH functional group - name ends in oic acid
Same element - different number of neutrons
M1V1 = M2V2

43. Acetate ion
C2H3O2?
Diamond - graphite - amorphous - fullerenes
M1V1 = M2V2
Black

44. What metal will react in hot water?
Magnesium
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Low pressures - high temperatures
Yellow to orange

45. Compounds with 18 carbons
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Moles of solute / kg solvent
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.

46. Color of Ni2+ solution
Green
V1/T1 = V2/T2
CO - produced from incomplete combustion - very toxic
Same molecule - different electron pair positions

47. Compounds with 1-4 carbons
Gases at room temperature - used for fuel
Two reactants combine to form a single product
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Green

48. If G is zero - what is happening in the reaction?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
COOH - ends in -oic acid
It is at equilibrium

49. Isotope
OH - alcohols - name ends in ol
The solute is dissolved in the solvent.
Same element - different number of neutrons
Stronger

50. Gibb's Free Energy equation
Strong acids - strong bases - soluble salts
DG = DH - TDS
ClO3?
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

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SAT Subject Test: Chemistry

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