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The Every Now and Then Table
The Name Game
Dont Over-React
Weights and Measures
I Dig Your Quantums.
Potpourri
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60
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3
10 pts
TIME
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ZnS
Zinc sulfide
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20 pts
TIME
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AgNO3
Silver nitrate
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30 pts
TIME
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Cu(II)SO4
Copper II sulfate
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40 pts
TIME
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Ba(ClO3)2
Barium chlorate
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50 pts
TIME
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Mn(OH)2
Manganese hydroxide
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60 pts
TIME
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Sb2(SO4)3
Antimony sulfate
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70 pts
TIME
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Sn(II)3(PO3)2
Tin II phoshpite
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10 pts
TIME
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the abbreviation is AMU
Atomic mass unit
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20 pts
TIME
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The abbreviation for it is PVC
Polyvinyl chloride
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30 pts
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It is the SI unit for temperature, abbreviated
K
Kelvin
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40 pts
TIME
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Chemistry terms correctly describing these three
arrow shots
Precise, but not accurate
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50 pts
TIME
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Type of bonding shown here
Ionic bonding
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60 pts
TIME
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It is the first name of this persons mother
Barbara
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70 pts
TIME
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The name of the campus shown here
Los Osos
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10 pts
TIME
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It is the minimum quantity of energy that can be
lost or gained by an atom
quatum
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20 pts
TIME
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The number of quantum numbers required to define
an orbital
four
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30 pts
TIME
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The name of the quantum number symbolized by n
Principle quantum number
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40 pts
TIME
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It states that it is impossible to determine
simultaneously both the position and velocity of
an electron
Heisenberg uncertainty principle
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50 pts
TIME
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Bands of light given off by an excited atom
Line-emission spectrum
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60 pts
TIME
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Says an electron occupies the lowest-energy
orbital that can receive it.
Aufbaugh principle
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70 pts
TIME
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No two electrons in the same atom can have the
same set of four quantum numbers
Pauli exclusion principle
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10 pts
TIME
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He is considered the father of the periodic
table
Dmitri Mendeleev
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20 pts
TIME
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Mendeleev ordered his periodic table by this now
we do it by atomic number
Atomic mass
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30 pts
TIME
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It states that the physical and chemical
properties of the elements are periodic functions
of their atomic numbers
Periodic law
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40 pts
TIME
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going from left to right across a period, atomic
radius does this
decreases
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50 pts
TIME
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They are the type of orbitals being filled in the
actinide and lanthanide series
f orbitals
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60 pts
TIME
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It is the electron configuration for aluminum
1s22s22p63s23p1
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70 pts
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it is defined as a measure of the ability of an
atom in a chemical compound to attract electrons
electronegativity
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10 pts
TIME
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it is the amount of space occupied by an object
volume
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20 pts
TIME
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It is the ratio of mass to volume
density
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30 pts
TIME
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Refers to the closeness of a measurement to the
correct or accepted value
accuracy
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40 pts
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The number of significant figures in 1023.030
7
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50 pts
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The number of significant digits in 1200000000
2
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60 pts
TIME
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State 125000000 in scientific notation
1.25 x 10 8
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70 pts
TIME
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State 0.0000030045 in scientific notation
3.0045 X 10-6
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10 pts
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Type of reaction A B ? AB
synthesis
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20 pts
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This type of reaction produces carbon dioxide and
water
Combustion rxn
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30 pts
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Name the type of reaction Zn3(PO4)2
Cu(II)(NO4)2 ? Zn(NO4)2 Cu(II)3(PO4)2
Double displacement (replacement)
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40 pts
TIME
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Two of the 5 signs of a chemical reaction
Evolution of Heat Evolution of Light Production
of a gas Production of a precipitate Color change
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50 pts
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This type of reaction A BX ? AX B
Single displacement (replacement)
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60 pts
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They are the whole numbers used in front of
chemical formulas to balance reactions
coefficients
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70 pts
TIME
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The type of reaction shown here H2SO4 2 NaOH ?
2 H2O Na2SO4
Acid-base
45

• Final exam
• Wednesday 100 multiple choice questions
• You may use
• 3x5 notecards, or your chapter notecards
• Calculator
• Periodic table

46

• A chemical change occurs when
• Dissolved minerals solidify to form a crystal
• Ethanol is purified through distillation
• Salt deposits form from evaporated sea water
• A leaf changes color

47

• A physical change occurs when a
• Peach spoils
• Copper bowl tarnishes
• Bracelet turns your wrist green
• Glue gun melts a glue stick

48

• The state of matter in which particles are
  rigidly held in fixed positions is the
• Gaseous state
• Liquid state
• Vaporous state
• Solid state

49

• Which element has properties most similar to
  those of sodium?
• Boron
• Calcium
• sulfur
• nitrogen

50

• To calculate the density of an object,
• Multiply its mass and its volume
• Divide its mass by its volume
• Divide its volume by its mass
• Divide its mass by its area

51

• 0.25 g is equivalent to
• 250 kg
• 250 mg
• 0.025 mg
• 0.025 kg

52

• If 1 inch equals 2.54 cm, how many centimeters
  equal 1 yard?
• 0.07 cm
• 14.17 cm
• 36 cm
• 91.4 cm

53

• A measurement is said to have good precision if
  it
• Agrees closely with an accepted standard
• Agrees closely with other measurements of the
  same quantity
• Has a small number of significant figures
• Has a large number o significant figures

54

• In division and multiplication, the answer must
  not have more significant figures than the
• Number in the calculation with fewest significant
  figures
• Number in the calculation with most significant
  figures
• Average number of significant figures in the
  calculation
• Total number of significant figures in the
  calculation

55

• The speed of light is 300,000 km/s. In
  scientific notation this speed is
• 3 X 105 km/s
• 3.00 X 105 km/s
• 3.0 X 106 km/s
• 3.00 X 106 km/s

56

• The result of dividing 107 by 10-3 is
• 10-4
• 102.5
• 104
• 1010

57

• The nucleus of an atom has all of the following
  characteristics EXCEPT that it
• Is positively charged
• b. Is very dense
• Contains nearly all of the atoms mass
• Contains nearly all of the atoms volume

58

• Chlorine has atomic number 17 and mass number 35.
  It has
• 17 protons, 17 electrons, and 18 neutrons
• 35 protons, 35 electrons, and 17 neutrons
• 17 protons, 17 electrons, and 52 neutrons
• 18 protons, 18 electrons, and 17 neutrons

59

• The mass of 1 mol of chromium (atomic mass 51.996
  amu) is
• 12 g
• 198 g
• 51.996 g
• 6.02 X 1023 g

60

• How many moles of atoms are in 50.15 g of mercury
  (atomic mass 200.59 amu)?
• 0.1001 mol
• 0.1504 mol
• 0.2500 mol
• 0.4000 mol

61

• The region outside the nucleus where an electron
  can most probably be found is the
• Electron configuration
• Quantum
• S sublevel
• Electron cloud

62

• Two electrons in the 1s orbital must have
  different spin quantum numbers to satisfy
• Hunds rule
• The magnetic rule
• The Pauli exclusion principle
• The aufbau principle

63

• Mendeleev noticed that properties of elements
  usually repeated at regular intervals when the
  elements were arranged in order of increasing
• Atomic number
• Density
• Reactivity
• Atomic mass

64

• Neutral atoms with an s2p6 electron configuration
  in the highest energy level are best classified
  as
• Metalloids
• Metals
• Nonmetals
• gases

65

• Within a group of elements, as the atomic number
  increases, the atomic radius
• Increases
• Remains approximately constant
• Decreases regularly
• Decreases, but not regularly

66

• The electrostatic attraction between ______ forms
  an ionic bond
• Ions
• Dipoles
• Electrons
• Orbitals

67

• The B-F bond in BF3 (electronegativity for B is
  2.0 for F is 4.0) is
• Polar covalent
• Ionic
• Nonpolar covalent
• Pure covalent

68

• Changing a subscript in a correctly written
  chemical formula
• Changes the number of moles represented by the
  formula
• Changes the charges on the other ions in the
  compound
• Changes the formula so that it no longer
  represents that compound
• Has no effect on the formula

69

• Name the compound Fe(NO2)2
• Iron (II) nitrate
• Iron (II) nitrite
• Ferric nitrate
• Ferrous nitride

70

• Chemical properties
• Include changes of state of a substance
• Include mass and color
• Include changes that alter the identity of a
  substance
• Can be observed without altering the identity of
  a substance

71

• Which of the following observations is
  quantitative?
• The liquid turns blue litmus paper red
• The liquid boils at 100 degrees C
• The liquid tastes bitter
• The liquid is cloudy

72

• According to Bohrs theory, an excited atom would
• Collapse
• Absorb photons
• Remain stable
• Radiate energy

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• If the atoms that share electrons have an unequal
  attraction for the electrons, the bond is called
• Nonpolar
• Polar
• Ionic
• dipolar