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

Which bond is the least polar?

A.As-Cl

B.Bi-Cl

C.P-Cl

D.N-Cl

What is D. N-Cl

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

Which compound contains both ionic and covalent bonds?

A.KI

B.CaCl2

C.CH2Br2

D.NaCN

What is D. NaCN

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