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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. Covalent-network / atomic solids
Stronger
4.5 to 8.3 - Red to blue
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
P1/V1 = P2/V2

2. Molecular solids
SO4²?
Stronger
Emission of electromagnetic energy after beta - positron - or alpha decay
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose

3. Tetrahedral
No
4 bonding - 109.5° - sp³ hybridization
Blue-green
PO4³?

4. If G is zero - what is happening in the reaction?
White
It is at equilibrium
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
NH2 functional group - name ends in -amide

5. Supersaturated solution
2 bonding - 180° - sp hybridization
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
Classified as strong bases but not very soluble.
Covalent

6. What 3 metals will react with cold water?
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
ClO3?
Lemon yellow
Potassium - Calcium - Sodium

7. Chlorate ion
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Two reactants combine to form a single product
Heat required to make a substance melt.
ClO3?

8. General properties of alloys
NH4?
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
NH2 functional group - name ends in -amide

9. If G is positive - is the reaction spontaneous?
Involves water
No
The solute is dissolved in the solvent.
Soluble except when containing alkaline earth metals

10. Noble gases
7th group - form salts - always exist as diatomic molecules - used in modern lighting
Yes
Substance can act either as an acid or a base
Extremely slow reactivity

11. Compounds with 12-18 carbons
6.0 to 7.6 - yellow to blue
3.1 - 4.4 - red to yellow
Soluble
Make up jet fuels and kerosene

12. Isoelectronic
Moles of solute / kg solvent
Two atoms with the same number of electrons
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Refract light as result of unpaired electrons - several oxidation states - ionic solutions are colored

13. Dalton's Law
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation
Pressure of mixture of gases equals some of individual gas pressures.
Make up jet fuels and kerosene

14. Carboxylic acid
Diamond - graphite - amorphous - fullerenes
COOH functional group - name ends in oic acid
Orientation of orbital in space
Black

15. Halogen properties
It is at equilibrium
Mixture of tin - copper - bismuth - and antimony
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
Moles / L

16. Silver bromide and silver iodide are used for
yellow
Lemon yellow
Defines shape of orbital
Photography

17. Brass
Mixture of copper and zinc
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Increases left and down
Low pressures - high temperatures

18. What metal will react in hot water?
Magnesium
Etching glass and frosting lightblubs
PV = nRT - R = .0821
3 bonding - 120° - sp² hybridization

19. Carbon dioxide gas properties
Light green
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

20. Alkali Metals
Classified as strong bases but not very soluble.
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
1st group - most reactive metal family - react violently with water - create basic solutions
Photography

21. Cl - Br - and I compounds are...
2nd group - fairly reactive - pastes are used in batteries
Substance can act either as an acid or a base
Soluble
Soluble except when containing Ag? - Hg2²? - or Pb²?

22. What are the allotropic forms of sulfur?
White
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Energy level - as it increases electrons are less bound to the nucleus
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.

23. Color of excited K+
Two atoms with the same number of electrons
Purple/pink
Acid to water
Colorless - odorless - low density - flammable - slightly soluble in water - diffuses more rapidly than any other gas - good reducing agent

24. Aldehydes
Blue
COH functional group - name ends in -al
No
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

25. Carbon monoxide
Increases left and down
Purple
CO - produced from incomplete combustion - very toxic
Red

26. Sigma bonds
Degrade the oxone layer
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond

27. Pi bonds
Low pressures - high temperatures
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Two compound react to form two new compounds
NH2 functional group - name ends in -amide

28. Decomposition reaction
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
A compound breaks into two parts
Gas pressure = atm pressure - height of mercury
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

29. F compounds are...
Soluble except when containing alkaline earth metals
More active element replaces less active element in a compound.
DTb = (Kb)(msolute)(i) - for water Kb is 0.51
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

30. Acids with more oxygen atoms are
Used as an antifreeze - used in gasoline - flammable - miscible with water - good solvent
Diamond - graphite - amorphous - fullerenes
Soluble
Stronger

31. Fusion
CO - produced from incomplete combustion - very toxic
Two atoms with the same number of electrons
Do not conduct electricity well
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)

32. Dipole-dipole forces (including hydrogen bonds)
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
R-O-R functional group - shorter chain ends in oxy - other is ane
Make up jet fuels and kerosene
NH4?

33. Magnetic quantum number (ml)
Orientation of orbital in space
Soluble except when containing alkaline earth metals
2 bonding - 1 nonbonding
4.184

34. Amine group
NH2 - ends in -amide
Glass and plastic
No two electrons can have the same set of 4 quantum numbers
Defines shape of orbital

35. What kind of bonds generally hold gases together?
Orange
Covalent
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Yes in thermo - no in electro

36. Chlorine gas
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
COOH functional group - name ends in oic acid
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Deadly - yellow-green - weapon

37. Examples of amorphous solids
Photography
Two atoms with the same number of electrons
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Glass and plastic

38. Oxides are insoluble and when reacted with water..
Nonmetal oxides form acids - metal oxides form bases
Periods 8 and 9 - lanthanides and actinides
Glass and plastic
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

39. Dilution equation
M1V1 = M2V2
Diatomic - fluorine is a gas - bromine is a liquid iodine is a solid - fluorine is most reactive - chlorine is an antibacterial agent
DTf = (Kf)(msolute)(i) - for water Kf is 1.86
Soluble except when containing alkaline earth metals

40. Hydrofluoric acid is used for
Mixture of iron and carbon
COOH functional group - name ends in oic acid
Etching glass and frosting lightblubs
Pressure of mixture of gases equals some of individual gas pressures.

41. Methanol
Miscible with water - flammable - used as fuel - poisonous
Blue
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

42. Nonmetals
Do not conduct electricity well
1st group - most reactive metal family - react violently with water - create basic solutions
COOH functional group - name ends in oic acid
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4

43. Alkaline metal oxides are...
Classified as strong bases but not very soluble.
Soluble except when containing Ag? - Hg2²? - or Pb²?
Yellow to orange
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)

44. Bromthymol blue: pH range and colors
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
6.0 to 7.6 - yellow to blue
Light green
Same formula - different structure

45. Amine
NH2 functional group - name ends in -amide
Orange
Between metal and non-metal - electronegativity difference greater than 1.7 - high melting points - solid state under standard conditions - electron is completely transferred
Stronger

46. Is removing an electron an exothermic or endothermic process?
Increased
Bright yellow
Endothermic
Most stable

47. Name the six strong acids
Light green
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules

48. Isotope
Purple/pink
Same element - different number of neutrons
React with water to form bases - react with acids to form hydrogen gas - more reactive down group
A compound breaks into two parts

49. Ionic solids
V1/T1 = V2/T2
Miscible with water - flammable - used as fuel - poisonous
Decreased
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl

50. Rare earth elements
Periods 8 and 9 - lanthanides and actinides
The solute is dissolved in the solvent.
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
White