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SAT Subject Test: Chemistry

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Answer 50 questions in 15 minutes.
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1. CO3²? - PO4³? - C2O4²? - CrO4²? - S²? - OH? - and O2 compounds are...
NH4?
1. Water solutions conduct electricity 2. Litmus is blue - phenolphthalein is pink 3. React with fats to form soaps
Soluble except when containing Ag? - Hg2²? - or Pb²?
Insoluble

2. Covalent-network / atomic solids
Potassium - Calcium - Sodium
Increase right and up
DG = DH - TDS
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite

3. Gibb's Free Energy equation
Lemon yellow
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
2 bonding - 1 nonbonding
DG = DH - TDS

4. Single Replacement / displacement reaction
Two reactants combine to form a single product
Emission of electromagnetic energy after beta - positron - or alpha decay
Deadly - yellow-green - weapon
More active element replaces less active element in a compound.

5. Isoelectronic
Decreased
White
Two atoms with the same number of electrons
Nonmetal oxides form acids - metal oxides form bases

6. If G is negative - is the reaction spontaneous?
4.5 to 8.3 - Red to blue
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
Yes

7. Spin quantum number (ms)
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
Gas pressure = atm pressure + height of mercury
Spin is +1/2 or -1/2 in an orbital

8. Noble gas properties
Most stable
6 bonding - 90° - sp³d2² hybridization
Two atoms with the same number of electrons
COOH functional group - name ends in oic acid

9. NO3? - ClO3? - ClO4? and CH3COO (acetate) compounds are...
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs
Energy level - as it increases electrons are less bound to the nucleus
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Soluble

10. Chlorine gas
Deadly - yellow-green - weapon
Degrade the oxone layer
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Endothermic

11. 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
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
V1/T1 = V2/T2
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

12. Carbonate ion
Acid to water
Same molecule - different electron pair positions
Blue-green
CO3²?

13. What qualifies as a strong base?
Orientation of orbital in space
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
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
Atom becomes more stable by emitting a positively charged electron when a proton becomes a neutron and positron - decreasing the atomic number by 1

14. What are the factors that affect reaction rate?
Concentration of reactants - temperature - presence of a catalyst - and physical state of the reactants
4.184
Orange
Mixture of copper and zinc

15. Fusion
It is at equilibrium
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Same formula - different structure

16. bronze
Mixture of iron and carbon
Defines shape of orbital
Mixture of copper - zinc - and other metals
DH = bonds broken - bonds formed

17. Phenolphthalein: pH range and colors
Liquid at room temperature - used to make gasoline and solvents
8.3 to 10.0 - colorless to pink
Two light nuclei combine to form a heavier - more stable nucleus (very exothermic)
Lemon yellow

18. Molecular solids
Stronger
Between neutral polar molecules - stronger polarity means stronger dipole-dipole forces - hydrogen bonds are between hydrogen and fluorine - oxygen - or nitrogen.
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
P1/V1 = P2/V2

19. Steel
Soluble
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
Mixture of iron and carbon
ClO3?

20. Compounds with 18 carbons
Soluble
Solid at room temperature
Liquid at room temperature - used to make gasoline and solvents
OH - alcohols - name ends in ol

21. Equation when using a barometer to calculate gas pressure.
Gas pressure = atm pressure - height of mercury
yellow
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
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

22. Properties of molecular crystals and liquids

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23. If G is positive - is the reaction spontaneous?
Properties of solutions that depend on the number of particles per solvent molecule
Moles of solute / kg solvent
Strong acids - strong bases - soluble salts
No

24. Complete combustion occurs when there is
A compound breaks into two parts
Excess oxygen
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger

25. Sterling silver
Mixture of silver and copper
Moles / L
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
760 mmHg = 760 torr = 1 atm = 101 -325 Pa

26. Sulfide color: Sb2S3
Orange
Blue-green
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
2 bonding - 1 nonbonding

27. pewter
Hydrocarbon burned in the presence of oxygen to form carbon dioxide and water
Mixture of tin - copper - bismuth - and antimony
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Moles / L

28. What kind of bonds generally hold gases together?
4.5 to 8.3 - Red to blue
Covalent
Result from sideways overlap of p orbitals - never occur unless a sigma bond is created first
Made of metal atoms - held together by metallic bonds - high melting points - can be malleable or hard - good conductors.

29. Ionic solids
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
C2H3O2?
COOH functional group - name ends in oic acid
No

30. Carbon dioxide gas properties
Colorless - odorless - used as fire extinguisher - when bubbled in lime water - the solution will become cloudy and calcium carbonate precipitates
White
NO3?
React with water to form bases - react with acids to form hydrogen gas - more reactive down group

31. Carboxylic acid group
Soluble
Covalently bonded molecules with covalent intermolecular bonds - hard - high melting points - poor conductors. Ex: diamond - graphite
COOH - ends in -oic acid
Spontaneous degeneration of an unstable atomic nucleus with the emission of radiation

32. General Properties of Organic Compounds
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Low melting points - nonpolar unless they have functional groups - nonconductors - exist in all states
Oxides and hydroxides of alkali metals and alkaline earth metals - H? - and CH3?
Two atoms with the same number of electrons

33. Name the six strong acids
HCl - HBr - HI - HNO3 - H2SO4 - HCLO4
Soluble except when containing Ag? - Hg2²? - or Pb²?
NH4?
1st group - most reactive metal family - react violently with water - create basic solutions

34. Properties of acids
Rhombic (yellow - brittle) - monoclinic (needle-shaped - yellow - waxy - translucent) - and amorphous (noncrystalline - dark - elastic)
Mixture of copper and zinc
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
Insoluble

35. Beta particle
CO3²?
COH functional group - name ends in -al
Excess oxygen
High speed electrons - increase atomic number by 1 - range of 12 cm - weak interactions - 100 ionizations per cm - low energy

36. What metal will react in hot water?
ClO3?
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
Magnesium
Soluble

37. Rare earth elements
COOH functional group - name ends in oic acid
Covalent
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
Periods 8 and 9 - lanthanides and actinides

38. Litmus: pH range and colors
Diamond - graphite - amorphous - fullerenes
R-CO-R functional group ends in -one - w/ number indicated where the double bonded oxygen is
760 mmHg = 760 torr = 1 atm = 101 -325 Pa
4.5 to 8.3 - Red to blue

39. London dispersion forces
Weak forces between nonpolar molecules and noble gas atoms when electron cloud becomes asymmetrical - dispersion forces are greater among larger nonpolar molecules
Lemon yellow
Two compound react to form two new compounds
Do not conduct electricity well

40. Carbon monoxide
CO - produced from incomplete combustion - very toxic
Soluble
No
BeH2 (only 2 valence pairs) - periods 4 and above can have more than 4 valence pairs

41. Bent
Degrade the oxone layer
2 bonding - 1 nonbonding
Yellow to orange
Liquid at room temperature - used to make gasoline and solvents

42. Fission
Solution where particles settle - can be separated - sometimes scatter light - usually not transparent
Increase right and up
A heavy nucleus splits into two nuclei - when bombarded by small particles (very exothermic)
Gold

43. SO4²? compounds are...
Classified as strong bases but not very soluble.
Liquid at room temperature - used to make gasoline and solvents
Soluble except when they include Ca²? - Sr²? - Ba²? - Ag²? - Pb²? - or Hg2²?
Yellow to orange

44. Amine
NH2 functional group - name ends in -amide
6.0 to 7.6 - yellow to blue
Energy level - as it increases electrons are less bound to the nucleus
Yes in thermo - no in electro

45. Nonmetals
Do not conduct electricity well
Made of positive and negative ions held together by electrostatic attractions. High melting points - brittle - poor conductors as solids. Ex: NaCl
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.
Covalent

46. What is the equation used for heat transfer problems?
Yellow
Q = mcDT
Covalent
Bright yellow

47. Sigma bonds
Q = mcDT
Two compound react to form two new compounds
Single bonds - result from overlap of two s orbitals - an s and p orbital - or two p orbitals - greatest overlap means stronger bond
C2H3O2?

48. Isotope
The solute is dissolved in the solvent.
Same element - different number of neutrons
More negative means easier to gain electrons - increases left - no change in groups - exception is noble gases who have positive electron affinities
6.0 to 7.6 - yellow to blue

49. General properties of alloys
Made of atoms or molecules held together by dipole forces - hydrogen bonds - or London dispersion forces. Low melting points - flexible - poor conductors. Ex: Sucrose
1. Lower melting point than components 2. Harder than components 3. If cooled slowly - particles are larger
Two reactants combine to form a single product
A compound breaks into two parts

50. Supersaturated solution
Solution heated - more solute added - then cooled. Solution holds more solute than theoretically possible - very unstable.
1. Electrolysis of water 2. passing steam over hot iron or through hot coke 3. decomposing natural gas (mostly methane) with heat and water
R-O-R functional group - shorter chain ends in oxy - other is ane
Mixture of tin - copper - bismuth - and antimony

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SAT Subject Test: Chemistry

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