Test your basic knowledge |

SAT Subject Test: Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. What metal will react in hot water?
Light 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
8.3 to 10.0 - colorless to pink
Magnesium

2. Gamma decay
C2H3O2?
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
2nd group - fairly reactive - pastes are used in batteries
Emission of electromagnetic energy after beta - positron - or alpha decay

3. What kind of bonds generally hold liquids together?
Properties of solutions that depend on the number of particles per solvent molecule
Mixture of silver and copper
Classified as strong bases but not very soluble.
Covalent

4. Rare earth elements
Yellow
Limited oxygen
Periods 8 and 9 - lanthanides and actinides
Covalent

5. Sulfide color: CdS
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
Magnesium
6 bonding - 90° - sp³d2² hybridization

6. What kind of bonds generally hold gases together?
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Two atoms with the same number of electrons
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Covalent

7. Color of excited Na+
Bright yellow
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
yellow
R-O-R functional group - shorter chain ends in oxy - other is ane

8. Brass
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
A compound breaks into two parts
Mixture of copper and zinc

9. Ammonium Ion
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
Pressure of mixture of gases equals some of individual gas pressures.
NH4?
Covalent

10. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
3 bonding - 1 nonbonding 107°
Orange
Degrade the oxone layer
Soluble

11. General properties of alloys
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
V1/T1 = V2/T2
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities

12. Hydrolysis reaction
Diamond - graphite - amorphous - fullerenes
Liquid at room temperature - used to make gasoline and solvents
Involves water
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

13. Chlorate ion
ClO3?
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
OH - alcohols - name ends in ol
Emission of electromagnetic energy after beta - positron - or alpha decay

14. Charles' Law
DH = bonds broken - bonds formed
Electrons are free to move through metal structure - high conductivity - ductile
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

15. What 3 metals will react with cold water?
Insoluble
Potassium - Calcium - Sodium
Electrons are free to move through metal structure - high conductivity - ductile
Orange

16. Beta particle
Mixture of copper - zinc - and other metals
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Moles of solute / kg solvent
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

17. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
4.5 to 8.3 - Red to blue
M1V1 = M2V2
3 bonding - 120° - sp² hybridization

18. Sulfide color: As2S3
Lemon yellow
Two atoms with the same number of electrons
Mixture of copper and zinc
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

19. Isotope
4.184
Solid at room temperature
Same element - different number of neutrons
Mixture of copper and zinc

20. Halogens
Acid to water
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Strong acids - strong bases - soluble salts
7th group - form salts - always exist as diatomic molecules - used in modern lighting

21. Define heat of fusion.
M1V1 = M2V2
PV = nRT - R = .0821
Heat required to make a substance melt.
Solid at room temperature

22. Phenolphthalein: pH range and colors
Covalent
8.3 to 10.0 - colorless to pink
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Photography

23. Principal quantum number (n)
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Extremely slow reactivity
Solid at room temperature
Energy level - as it increases electrons are less bound to the nucleus

24. Ketone
V1/T1 = V2/T2
PO4³?
3 bonding - 120° - sp² hybridization
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

25. Azimuthal quantum number (l)
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
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Strong acids - strong bases - soluble salts
Defines shape of orbital

26. Hydroxyl group
Light green
CO3²?
OH - alcohols - name ends in ol
Glass and plastic

27. Halogen properties
Diamond - graphite - amorphous - fullerenes
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
M1V1 = M2V2
SO4²?

28. Supersaturated solution
Limited oxygen
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
2 bonding - 180° - sp hybridization

29. Silver bromide and silver iodide are used for
Two reactants combine to form a single product
White
M1V1 = M2V2
Photography

30. Octahedral
Green
Soluble
6 bonding - 90° - sp³d2² hybridization
Soluble

31. List equivalent pressure values for mmHg - torr - atm - and Pa
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Covalent
Properties of solutions that depend on the number of particles per solvent molecule

32. pewter
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
3 bonding - 1 nonbonding 107°
3.1 - 4.4 - red to yellow
Mixture of tin - copper - bismuth - and antimony

33. Alpha particle
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
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
OH functional group - name ends in -ol

34. Fission
5 bonding - 90° and 120° - sp³d hybridization
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
2nd group - fairly reactive - pastes are used in batteries
Pressure of mixture of gases equals some of individual gas pressures.

35. Electronegativity
Gas pressure = atm pressure - height of mercury
Mixture of copper and zinc
Increase right and up
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states

36. Tetrahedral
Same element - different number of neutrons
P1/V1 = P2/V2
Gold
4 bonding - 109.5° - sp³ hybridization

37. Trigonal planar
Limited oxygen
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.
Gas pressure = atm pressure - height of mercury
3 bonding - 120° - sp² hybridization

38. If G is negative - is the reaction spontaneous?
Yes
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Liquid at room temperature - used to make gasoline and solvents
Orientation of orbital in space

39. Methanol
Miscible with water - flammable - used as fuel - poisonous
OH functional group - name ends in -ol
Blue
Properties of solutions that depend on the number of particles per solvent molecule

40. Equation when using a barometer to calculate gas pressure.
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
Gas pressure = atm pressure - height of mercury
4.184
Electrons are free to move through metal structure - high conductivity - ductile

41. Electron affinity
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Endothermic
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

42. Carboxylic acid group
Soluble
Gases at room temperature - used for fuel
COOH - ends in -oic acid
Q = mcDT

43. Color of CrO7²? solution
Blue
White
Orange
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

44. Exceptions to the octet rule
Acid to water
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Diamond - graphite - amorphous - fullerenes
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

45. Magnetic quantum number (ml)
Yes
OH functional group - name ends in -ol
Lemon yellow
Orientation of orbital in space

46. Alchohols
White
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Decreased
OH functional group - name ends in -ol

47. What are the factors that affect reaction rate?
4.184
Energy level - as it increases electrons are less bound to the nucleus
Glass and plastic
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants

48. Litmus: pH range and colors
Nonmetal oxides form acids - metal oxides form bases
OH - alcohols - name ends in ol
Two atoms with the same number of electrons
4.5 to 8.3 - Red to blue

49. If G is positive - is the reaction spontaneous?
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Soluble
Potassium - Calcium - Sodium
No

50. What qualifies as a strong base?
It is at equilibrium
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Blue
P1/V1 = P2/V2