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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. Ethanol
2 bonding - 1 nonbonding
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Degrade the oxone layer

2. Beta particle
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Involves water
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy
Mixture of iron and carbon

3. List equivalent pressure values for mmHg - torr - atm - and Pa
Increased
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
P1/V1 = P2/V2

4. Sulfide color: CuS - HgS - and PbS
NH2 - ends in -amide
Black
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

5. Rare earth elements
Diamond - graphite - amorphous - fullerenes
Two atoms with the same number of electrons
4 bonding - 109.5° - sp³ hybridization
Periods 8 and 9 - lanthanides and actinides

6. Halogen properties
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Limited oxygen
Soluble except when containing alkaline earth metals
Blue-green

7. Formula for calculating enthalpy change with bond energies
DH = bonds broken - bonds formed
6 bonding - 90° - sp³d2² hybridization
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
DG = DH - TDS

8. Radioactivity
Magnesium
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Potassium - Calcium - Sodium

9. What are the allotropic forms of sulfur?
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
CO3²?
Defines shape of orbital
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent

10. Carboxylic acid
Deadly - yellow-green - weapon
COOH functional group - name ends in oic acid
Moles of solute / kg solvent
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water

11. Equation when using a manometer to calculate gas pressure - and the gas has a higher pressure than the atmosphere
3 bonding - 1 nonbonding 107°
Gas pressure = atm pressure + height of mercury
Rate of effusion A / Rate of effusion B = sq. root of molar mass B / sq. root of molar mass A
Make up jet fuels and kerosene

12. Combustion reaction
Light green
Glass and plastic
Etching glass and frosting lightblubs
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water

13. Pi bonds
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
2 bonding - 1 nonbonding
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Liquid at room temperature - used to make gasoline and solvents

14. Dalton's Law
CO3²?
Photography
Mixture of silver and copper
Pressure of mixture of gases equals some of individual gas pressures.

15. Compounds with 5-10 carbons
Increased
Liquid at room temperature - used to make gasoline and solvents
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
1st group - most reactive metal family - react violently with water - create basic solutions

16. Hydrogen gas properties
V1/T1 = V2/T2
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Do not conduct electricity well

17. Exceptions to the octet rule
More active element replaces less active element in a compound.
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
4.5 to 8.3 - Red to blue
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

18. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
Insoluble
Miscible with water - flammable - used as fuel - poisonous
COOH - ends in -oic acid
Light green

19. Metallic bonds
Low pressures - high temperatures
Defines shape of orbital
PO4³?
Electrons are free to move through metal structure - high conductivity - ductile

20. What kind of bonds generally hold gases together?
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Covalent
1st group - most reactive metal family - react violently with water - create basic solutions

21. Define heat of fusion.
Red
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
P1/V1 = P2/V2
Heat required to make a substance melt.

22. Color of excited Cu2+
Heat required to make a substance melt.
Blue-green
Soluble
Gas pressure = atm pressure - height of mercury

23. Oxides are insoluble and when reacted with water..
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
Nonmetal oxides form acids - metal oxides form bases
Moles of solute / kg solvent

24. Bromthymol blue: pH range and colors
More active element replaces less active element in a compound.
Diamond - graphite - amorphous - fullerenes
6.0 to 7.6 - yellow to blue
Mixture of iron and carbon

25. Isoelectronic
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.
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Two atoms with the same number of electrons
yellow

26. Sterling silver
Mixture of silver and copper
8.3 to 10.0 - colorless to pink
Etching glass and frosting lightblubs
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl

27. Alkali metal properties
Orientation of orbital in space
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

28. Resonance structures
Moles / L
Increased
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Same molecule - different electron pair positions

29. Equation when using a barometer to calculate gas pressure.
Gas pressure = atm pressure - height of mercury
Nonmetal oxides form acids - metal oxides form bases
COOH functional group - name ends in oic acid
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

30. Colligative properties
3 bonding - 1 nonbonding 107°
5 bonding - 90° and 120° - sp³d hybridization
Properties of solutions that depend on the number of particles per solvent molecule
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

31. Alpha particle
DH = bonds broken - bonds formed
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
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
3 bonding - 120° - sp² hybridization

32. Freezing point depression formula
COOH - ends in -oic acid
4.184
Substance can act either as an acid or a base
DTf = (Kf)(msolute)(i) - for water Kf is 1.86

33. Coal
No
Solid at room temperature
PV = nRT - R = .0821
Composed of hydrocarbons - sulfur - oxygen - and nitrogen. When combusted - sulfur becomes SO2

34. Ester
Orange
R-CO-O-R functoinal group - ends in ate - shortest R has a branch name ending in -yl
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Spin is +1/2 or -1/2 in an orbital

35. Anhydride
4 bonding - 109.5° - sp³ hybridization
Covalent
Heat required to make a substance melt.
Oxide that reacts with water to form either an acid or a base

36. General Properties of Organic Compounds
Purple
Moles of solute / kg solvent
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Diamond - graphite - amorphous - fullerenes

37. What is the ideal gas law?
Mixture of copper - zinc - and other metals
PV = nRT - R = .0821
COOH - ends in -oic acid
Two reactants combine to form a single product

38. When a reaction is endothermic - the entropy is
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Extremely slow reactivity
Increased

39. Name the six strong acids
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
6 bonding - 90° - sp³d2² hybridization
CO3²?
Two compound react to form two new compounds

40. Ionization energy
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Increases right and up - drops when electron pairing first occurs (p4) - drop from s block to p block
4 bonding - 109.5° - sp³ hybridization
Solid at room temperature

41. Acetate ion
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent
Periods 8 and 9 - lanthanides and actinides
Acid to water
C2H3O2?

42. What is the second law of thermodynamics?
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
Soluble
Disordered systems with higher entropies are favored
Light green

43. Color of excited Fe3+
Gold
Yes
The solute is dissolved in the solvent.
Strong acids - strong bases - soluble salts

44. What is the equation used for heat transfer problems?
1st group - most reactive metal family - react violently with water - create basic solutions
Q = mcDT
yellow
COOH functional group - name ends in oic acid

45. Petroleum
Mostly composed of hydrocarbons - refined by separating it into different boiling points of its components
Same formula - different structure
Orange
Do not conduct electricity well

46. Spin quantum number (ms)
Light green
Disordered systems with higher entropies are favored
Spin is +1/2 or -1/2 in an orbital
Gas pressure = atm pressure - height of mercury

47. Litmus: pH range and colors
Yellow to orange
Mixture of copper - zinc - and other metals
Potassium - Calcium - Sodium
4.5 to 8.3 - Red to blue

48. Alkali metal compounds and NH4? compounds are...
Gases at room temperature - used for fuel
Covalent
No
Soluble

49. Complete combustion occurs when there is
Excess oxygen
Diamond - graphite - amorphous - fullerenes
Electrons are free to move through metal structure - high conductivity - ductile
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)

50. If G is zero - what is happening in the reaction?
Etching glass and frosting lightblubs
It is at equilibrium
COOH - ends in -oic acid
Excess oxygen

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SAT Subject Test: Chemistry

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