Bonding I
Bonding II
Gases
Misc.
Misc.
100
Explain, in terms of bonds and energy, what occurs during the following reaction:
O + O --> O2
What is energy is released and bonds are broken
100
Conductivity in a metal results from the metal atoms having
A.High ionization energy
B.High electronegativity
C.Highly mobile electrons in the valence shell
D.Highly mobile protons in the nucleus
What is C. highly mobile electrons in the valence shell
100
Kinetic molecular theory states that all particles of an ideal gas are
A.colliding without transferring energy
B.in random, constant, straight-line motion
C.Arranged in a regular geometric pattern
D.Separated by small distances relative to their size
What is B. in random, constant, straight-line motion
100
Which statement describes a chemical property of silicon?
A.Silicon has a blue gray color
B.Silicon is a brittle solid at 20.oC
C.Silicon melts at 1414oC
D.Silicon reacts with fluorine
What is D. silicon reacts with Fluorine
100
At STP, which 2.0-gram sample of matter uniformly fills a 340-milliliter closed container?
A.Br2(l)
B.Xe(g)
C.Fe(NO3)2(s)
D.KCl(aq)
What is B. Xe(g)
200
Give an example of a network solid.
What is:
Diamond
Graphite
SiO2
200
Under which conditions does a A real gas behave least like an ideal gas?
What are low temperature and high pressure
200
At which point do a liquid and a solid exist at equilibrium?
A.sublimation point
B.melting point
C.vaporization point
D.boiling point
What is B. the Melting Point
200
What quantity of heat is released when 44.0g of liquid water at 0oC freezes to ice at the same temperature? [units needed]
What is 14,700 J
300
Draw the Lewis dot structure for KCl
300
When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid will
A.Freeze
B.Boil
C.Melt
D.Condense
What is B. boil
300
This heating curve represents a sample of a substance starting as a solid below its melting point. Describe the potential and average kinetic energy of the particles in this sample during interval DE.
What is PE increases and avg KE remains the same
300
Compared to an electron in the first electron shell of an atom, an electron in the third shell of the same atom has?
A.Less mass
B.Less Energy
C.More mass
D.More Energy
What is D. more energy
400
A solid substance was tested in the laboratory . The test results are listed below:
•Dissolves in water
•Is an electrolyte
•Melts at a high temperature
The solid substance has what type of bonds
What are ionic bonds
400
Identify the type of bond below:
What is a coordinate covalent bond.
400
Which temperature change would cause the volume of a sample of an ideal gas to double when the pressure of the sample remains the same?
1) from 200ºC to 400ºC
2) from 400ºC to 200ºC
3) from 200 K to 400 K
4) from 400 K to 200 K
What is 3) from 200 K to 400 K
400
Write an electron configuration for calcium in the excited state
What is 2-8-7-3 or 2-8-7-2-1
400
Which trends are observed as each of the elements within Group 15 on the periodic table are considered from top to bottom?
A.Their metallic properties decrease and their atomic radii decrease.
B.Their metallic properties decrease and their atomic radii increase.
C.Their metallic properties increase and their atomic radii decrease.
D.Their metallic properties increase and their atomic radii increase.
What is D. their metallic properties increase and their atomic radii increase.
500
Draw the structural formula for a molecule of nitrogen
500
Identify the shape and MOLECULAR polarity of CO2.
What are linear and non-polar
500
Which sample would have the same number of molecules as 11.2L of He(g) at 273K and 202kPa?
1) 11.2L of N2(g) at 300K and 202kPa
2) 22.4L of Ne(g) at 546K and 404kPa
3) 11.2L of CH4(g) at 273K and 202kPa
4) 22.4L of H2(g) at 546K and 404kPa
What is 3) 11.2L of CH4(g) at 273K and 202kPa
500
Describe, in terms of both electrons and energy state, how the light represented by the spectral lines is produced.
What is
—Different colors of light are produced when electrons return from higher energy states to lower energy states.
—Light energy can be emitted when electrons in excited atoms return to lower shells.
—Electrons release energy as they move toward the ground state.
500
Explain, in terms of electrons, why the ionic radius of a Group 2 element is smaller than its atomic radius.
What is
– The valence electron shell of a Group 2 atom is lost when it becomes an ion.
– A Group 2 ion has two fewer electrons than the atom from which it was formed