Transcript Physics Jeopardy 1st Semester Review

Chemistry Tri A Review
Unit 1
Icy
slopes
Unit 2
Hang
Ten
Unit 2
Be
Trendy
Unit 3
Ironic,
isn’t it?
Mixed
Bag
Work it
200
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600
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Unit 1
200
• How many significant figures are in the
measurement 0.0032? 40500? Convert
these numbers to scientific notation
– 2, 3
– 3.2 x 10-3, 4.05 x 104
Unit 1
400
• A tentative answer to a scientific
question is called? What is the variable?
The experimental control
– The hypothesis
– The one factor being tested
– Keeps all conditions constant
Unit 1
600
• Hydrogen has three isotopes H-1, H-2
and H-3. Given the average atomic
mass is 1.01, what is the most common
isotope of hydrogen? What is Mass
Defect?
– H-1
– Mass lost during a nuclear reaction
Unit 1
800
• All atoms of the same elements have
the same number of? Isotopes of the
same element vary in their numbers of.
What are the relative AMU of protons,
neutrons and electrons?
– Protons
– Neutrons and atomic mass
– 1, 1, 0
Unit 1
1000
• Absolute zero is what number in Kelvin?
In Celsius? At what temperature does
water boil in Celsius? In Kelvin?
– 0, -273C
– 100C, 373K
Unit 2
200
• A hertz is the same as? How is
wavelength measured?
– Cycle/second = s-1
– Distance between corresponding points on
consecutive waves
Unit 2
400
• Light has properties of? What is the
speed of light?
– Particles and waves
– 3.00 x 108 m/s
Unit 2
600
• What is the Heissenberg Uncertainty
Principal?
– Can’t measure position and momentum of
an electron simultaneously.
Unit 2
800
• For an electron to move from ground to
excited state what must be absorbed?
When is a line spectrum is produced?
– Energy
– When an electron falls back down to a
lower energy state.
Unit 2
1000
• What is the formula for energy of a
photon? For wavelength?
– E=hv
Energy (J) = h(6.6262 x 10-34 Js) x v(s-1)
• Lambda=c/v Wavelength (m) = c(3.00 x 108 m/s) /
v(s-1)
Unit 2
200
• How many electrons in any given orbital?
What are the d and f blocks called? How
many orbitals in the s, p, d and f. How many
electrons? What are the shapes of the s and
p orbitals?
–
–
–
–
–
2
Transition and inner transition metals
1,3,5,7
2,6,10,14
Sphere and dumbbell
Unit 2
400
• What are the vertical columns in the
periodic table called? The horizontal
rows? What is the least reactive group?
The most reactive metal group? The
most reactive nonmetals group?
– Groups; periods
– Noble gases
– Alkali
– Halogens
Unit 2
600
• What happens to reactivity in the metals as
you move down a group? What is the most
reactive metal? nonmetal? Why? What
happens to AR as you move down a group
and from R to L on the PT?
– Increases
– Fr largest atomic radius
– F smallest AR with the highest Electronegativity
and affinity
– Increases
Unit 2
800
• Which group has the highest ionizing
energy? Give the charges attained by
the elements of each group. What rule
describes how many electrons an atom
will gain or lose?
– Noble gases
– 1+, 2+, 3+ 4+/-, 3-, 2-, 1-, 0
– Octet rule
Unit 2
1000
• State the Atomic Law. Arrange the
following ions in order of increasing size
Li, Li-, Li+
– Properties of elements reoccur periodically
when arranged in order of increasing
atomic number
– Li+, Li, Li-
Unit 3
200
• What is happening to the electrons in
an ionic bond? Which groups elements
of the periodic table create ionic bonds?
Why?
– Give/take
– Metal to non metal
– Large difference in electronegativities.
Unit 3
400
• What are some characteristics of ionic
compounds
– High MP, brittle(s), Conduct electricity(aq)
Unit 3
600
• What is a cation? Which type of
elements form cations? What is an
anion? Which group of elements from
anions
– + ion, metals
– - ion, non metals
Unit 3
800
• What type of elements create covalent
bonds? What do you call a covalent
bond with a charge?
– Non metal to non metal
– Polyatomic
Unit 3
1000
• What are the formulas for phosphate?
Carbonate? Sulfate?
– PO4 3– CO3 2– SO4 2-
Mixed Bag
200
• Write the complete electron
configuration for Cl. Write the
abbreviated electron configuration for P
– 1s2 2s2 2p6 3s2 3p5
– (Ne) 3s2 3p3
Mixed Bag
400
• How would you name CI5? Write the
formula for sodium oxide
– Carbon penta Iodide
– Na2O
Mixed Bag
600
• Write the formula for carbonic acid. For
hydrobromic acid
– H2CO3
– HBr
Mixed Bag
800
• Give the number of protons, neutrons,
electrons, atomic mass, atomic number
and net charge for 9Be 2+
– 4, 5, 2, 9, 4, 2+
Mixed Bag
1000
• What type of mixture is salt water? Salt
and pepper. What is the next highest
energy level after 3d? According to
Bohr, how do electrons circle the
nucleus?
– Homogeneous, heterogeneous
– 4p
– Specific allowed orbits
Work it
200
• Give an example of a energy level that
could never exist (example 0s)
– 1p, 2d, 3f
Work it
400
• Convert 1 mg to micrograms and
express in scientific notation
– 1 x 103ug
Work it
600
• Write the formula for Copper II
Carbonate.
– CuCO3
Work it
800
• Give the symbols for mercury, silver,
lead, gold, potassium, tin and beryllium
– Hg, Ag, Pb, Au, K, Sn, Be
Work it
1000
• Calculate the frequency and energy of a
wave of 750nm? What is the formula for
calculating average atomic mass given
the fractional abundance of the isotopes
– 4.0 x 1014 s-1
– 2.7 x 10 –19 J
– (% x M1) + (% x M2) ……
Chapter 7&8
200
• In a circle, what physics concept is
thought of as linear speed?
– tangential speed
Chapter 7&8
400
• What is confused with centrifugal force
in rotational motion?
– inertia
Chapter 7&8
600
• Work in a circle is called?
– torque
Chapter 7&8
800
• The constant of Newton’s Universal Law
of Gravitation is?
– 6.67 x 10-11 Nm2/kg2
Chapter 7&8
1000
• Dan has a mass of 83.2 kg and Nate
has a mass of 57.3 kg. What is the
gravitational force between them if they
are sitting .800 m apart?
– 5.00 x 10-7 N
Final Jeopardy
• State Newton’s Third Law
– For every action, there is an equal and
opposite reaction.