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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. Chlorofluorocarbons
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
Glass and plastic
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

2. Positron emission
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Covalent
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
DH = bonds broken - bonds formed

3. Formula for calculating enthalpy change with bond energies
Do not conduct electricity well
yellow
DH = bonds broken - bonds formed
Gas pressure = atm pressure + height of mercury

4. Charles' Law
V1/T1 = V2/T2
Extremely slow reactivity
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Increases left and down

5. What are the allotropic forms of sulfur?
COH functional group - name ends in -al
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
21% of atmosphere - colorless - odorless - supports combustion reactions
Substance can act either as an acid or a base

6. Name the six strong acids
Purple
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

7. amphoteric
Substance can act either as an acid or a base
Same element - different number of neutrons
3 bonding - 120° - sp² hybridization
Orange

8. Sterling silver
DH = bonds broken - bonds formed
Mixture of silver and copper
Endothermic
Q = mcDT

9. Complete combustion occurs when there is
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
Moles of solute / kg solvent
Excess oxygen
Increased

10. Alchohols
OH functional group - name ends in -ol
4 bonding - 109.5° - sp³ hybridization
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Light green

11. Properties of ionic substances

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12. Define heat of fusion.
Do not conduct electricity well
Extremely slow reactivity
Heat required to make a substance melt.
Purple/pink

13. Color of CrO7²? solution
Covalent
Orange
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Decreased

14. Bromthymol blue: pH range and colors
6.0 to 7.6 - yellow to blue
Bright yellow
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
Purple/pink

15. Dipole-dipole forces (including hydrogen bonds)
Decreased
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Q = mcDT
Stronger

16. Compounds with 1-4 carbons
Gases at room temperature - used for fuel
Yellow to orange
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Decreased

17. Trigonal pyramidal
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
5 bonding - 90° and 120° - sp³d hybridization
Blue
3 bonding - 1 nonbonding 107°

18. Color of excited Li+ - Sr2+ - Ca2+
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Red
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Moles / L

19. Phosphate ion
Insoluble
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
PO4³?
Bright yellow

20. Ketone
2 bonding - 1 nonbonding
Limited oxygen
7th group - form salts - always exist as diatomic molecules - used in modern lighting
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is

21. Decomposition reaction
3 bonding - 1 nonbonding 107°
Defines shape of orbital
A compound breaks into two parts
Gas pressure = atm pressure - height of mercury

22. Anhydride
P1/V1 = P2/V2
Oxide that reacts with water to form either an acid or a base
Mixture of tin - copper - bismuth - and antimony
3 bonding - 120° - sp² hybridization

23. Allotropic forms of carbon
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Diamond - graphite - amorphous - fullerenes
3.1 - 4.4 - red to yellow
Extremely slow reactivity

24. Sulfide color: Sb2S3
Orange
OH functional group - name ends in -ol
Spin is +1/2 or -1/2 in an orbital
PV = nRT - R = .0821

25. Steel
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Involves water
Mixture of iron and carbon
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

26. Color of Cu2+ solution
COOH - ends in -oic acid
Blue
Purple/pink
P1/V1 = P2/V2

27. Trigonal planar
3 bonding - 120° - sp² hybridization
NO3?
Etching glass and frosting lightblubs
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

28. Colloid
Disordered systems with higher entropies are favored
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
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Purple

29. Carbonate ion
CO3²?
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Purple
Potassium - Calcium - Sodium

30. Sigma bonds
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Purple
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

31. Color of Fe3+ solution
Yellow to orange
21% of atmosphere - colorless - odorless - supports combustion reactions
SO4²?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps

32. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
Lemon yellow
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Soluble
Substance can act either as an acid or a base

33. Alkaline metal oxides are...
yellow
NH4?
Classified as strong bases but not very soluble.
Soluble except when containing alkaline earth metals

34. Molecular solids
Gases at room temperature - used for fuel
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1
Extremely slow reactivity

35. Radioactivity
It is at equilibrium
Properties of solutions that depend on the number of particles per solvent molecule
P1/V1 = P2/V2
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

36. Linear
Electrons are free to move through metal structure - high conductivity - ductile
2 bonding - 180° - sp hybridization
6 bonding - 90° - sp³d2² hybridization
Purple

37. Hydroxyl group
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
OH - alcohols - name ends in ol

38. Alkali metal properties
Yes in thermo - no in electro
4.5 to 8.3 - Red to blue
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
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

39. What kind of bonds generally hold liquids together?
Covalent
21% of atmosphere - colorless - odorless - supports combustion reactions
No two electrons can have the same set of 4 quantum numbers
Miscible with water - flammable - used as fuel - poisonous

40. Alkaline earth metals
2nd group - fairly reactive - pastes are used in batteries
6.0 to 7.6 - yellow to blue
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Mixture of tin - copper - bismuth - and antimony

41. Covalent-network / atomic solids
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
No two electrons can have the same set of 4 quantum numbers
Properties of solutions that depend on the number of particles per solvent molecule
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?

42. Hydrogen gas properties
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
R-O-R functional group - shorter chain ends in oxy - other is ane
P1/V1 = P2/V2
Increase right and up

43. Ionic solids
Degrade the oxone layer
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
Soluble except when containing Ag? - Hg2²? - or Pb²?

44. Pauli exclusion principle
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.
No two electrons can have the same set of 4 quantum numbers
SO4²?

45. Noble gas properties
Same molecule - different electron pair positions
Blue-green
Orange
Most stable

46. Chlorine gas
Deadly - yellow-green - weapon
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Covalent

47. Dilution equation
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Solid at room temperature
NO3?
M1V1 = M2V2

48. Molarity
Moles / L
Soluble
Gases at room temperature - used for fuel
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

49. What metal will react in hot water?
Solid at room temperature
Pressure of mixture of gases equals some of individual gas pressures.
Do not conduct electricity well
Magnesium

50. Tetrahedral
Gas pressure = atm pressure - height of mercury
4 bonding - 109.5° - sp³ hybridization
Increase right and up
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

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SAT Subject Test: Chemistry

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