60 Questions
How is a covalent bond represented in Lewis structures?
As dots between atoms
What electron configuration imparts special stability to noble gas elements?
Eight electrons in the outermost shell
What determines the chemistry of main-group elements?
The tendency to mimic noble gases
In Kekulé structures, how is a two-electron covalent bond indicated?
As a bold line between atoms
What results in a stable molecule according to the text?
Having eight dots for main-group atoms and two for hydrogen
What is the role of hydrogen in Lewis structures?
To represent its 1s electron with a dot
How many valence electrons does Carbon have?
Four
How many bonds does Hydrogen typically form?
One
Why does Carbon need to form four bonds?
To reach the neon configuration
What is the spatial orientation of the four C-H bonds in methane?
Tetrahedral
What happens when an s orbital hybridizes with three p orbitals?
It forms sp3 hybrid orbitals
What does the superscript 3 in sp3 hybrid orbitals represent?
The number of each type of atomic orbital combined to form the hybrid
What is the angle formed by each H - C - H bond in sp3 hybrid orbitals?
109.5°
Which type of hybrid orbitals result in unsymmetrical orbitals about the nucleus?
Sp2 hybrid orbitals
How many electron pairs are shared between atoms in a triple bond?
Three
Which type of hybrid orbitals form a σ bond by head-on overlap?
Sp2 hybrid orbitals
What is the structure of acetylene (HC ≡ CH) in terms of its carbon-carbon bond?
Triple bond
Which type of hybrid orbitals have an angle of 120° between the orbitals?
Sp2 hybrid orbitals
What is the special property of carbon that allows it to form a diverse range of compounds?
It can share four valence electrons and form four strong covalent bonds.
Why is carbon unique compared to other elements?
It can form long chains and rings by bonding to other carbon atoms.
What is the overall charge of an atom?
Neutral
Which subatomic particles are found in the nucleus of an atom?
Protons and neutrons
What allows carbon to form compounds ranging from simple methane to complex DNA?
Its ability to bond to one another, forming long chains and rings.
What has modern chemistry allowed scientists to do with organic compounds?
Design and synthesize new organic compounds in the laboratory.
What type of bond is formed by the combination of an sp2–sp2 σ bond and a 2p–2p π bond?
Pi bond
How many electrons are shared in the formation of a carbon–carbon double bond?
Four electrons
What type of hybrid orbital is needed to account for the triple bond in acetylene, H-C ≡ C-H?
sp
When two sp-hybridized carbon atoms approach each other, what type of bond is formed by the overlap of their sp hybrid orbitals?
Sigma bond
What happens when the pz orbitals from each carbon atom overlap during bonding?
Formation of pi bond
In sp hybridization, what is the orientation between the two resulting sp orbitals?
180 degrees apart
Sp3 hybrid orbitals form stronger bonds than unhybridized s or p orbitals.
True
The angle formed by each H - C - H bond in sp3 hybrid orbitals is 120°.
False
Ethylene contains a carbon–carbon triple bond.
False
In sp2 hybridization, three sp2 hybrid orbitals result and one 2p orbital remains unchanged.
True
The three sp2 orbitals lie in a plane at angles of 180° to one another.
False
When two carbons with sp2 hybridization approach each other, they form a σ bond by sp2–sp2 side-on overlap.
False
Hydrogen forms two covalent bonds because it has two valence electrons.
False
Lithium fluoride is formed by the transfer of one electron from fluorine to lithium.
False
Ionic bonding occurs when valence electrons are completely transferred between atoms.
True
Carbon forms four covalent bonds due to needing four additional valence electrons to reach the neon configuration.
True
Covalent bonds result from the sharing of protons between atoms.
False
In methane (CH4), all four C-H bonds are identical in spatial orientation.
True
Sp3 hybrid orbitals are symmetrical about the nucleus.
False
Energy is released from the chemical system when a bond is broken.
False
Carbon typically forms five bonds in its compounds.
False
The superscript 3 in sp3 hybrid orbitals indicates how many electrons occupy the hybrid orbital.
False
The tetrahedral orientation of sp3 hybrid orbitals results from the combination of an s orbital and two p orbitals.
False
Atoms bond together because the resulting compound is less stable than the separate atoms.
False
Carbon can form a triple bond by sharing six electrons.
True
Sp hybrid orbitals result from the combination of a carbon 2s orbital with two p orbitals.
False
When two sp-hybridized carbon atoms approach each other, sp orbitals overlap to form a strong pi bond.
False
The combination of an sp2–sp2 σ bond and a 2p–2p π bond results in the sharing of six electrons.
False
Two sp hybrid orbitals are oriented 180° apart on the y-axis.
False
Py orbitals from each carbon overlap to form a py–py π bond by sideways overlap.
True
A stable molecule is formed when a noble-gas configuration is achieved for all the atoms.
True
Covalent bonds are indicated as a line drawn between atoms in Lewis structures.
False
Carbon has four dots in its Lewis structure, representing its 1s electron.
False
An octet of electrons in the valence shell provides special stability to noble gas elements.
True
Kekulé structures represent covalent bonds as dots in Lewis structures.
False
Main-group elements do not tend to take on the electron configuration of the nearest noble gas.
False
Explore the unique properties of carbon that make it the foundation of organic chemistry. Learn about carbon's ability to share four valence electrons, form strong covalent bonds, and create diverse compounds through chain and ring formations.
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