18 Questions
What is electronegativity a measure of?
The attraction of an atom for electrons in a bond
In a polar covalent bond, electrons are pulled towards which type of element?
The element with greater electronegativity
When do atoms form a nonpolar bond?
When the electronegativities of the two atoms are equal or similar
What is indicated by the symbol δ+ in a bond?
Electrons are pulled away from the atom
How is the polarity of a molecule determined?
By the polarity of the individual bonds and the molecular shape
What is a common characteristic of nonpolar molecules?
Individual bond dipoles that do not cancel
What is the number of electrons in a triple bond?
Six
Which element needs only two electrons in bonding?
Hydrogen
What is the purpose of resonance structures?
To spread out lone pairs and electron pairs in multiple bonds
What is the term for the theory used to determine the shape around a given atom?
VSEPR Theory
What happens when drawing Lewis structures for polyatomic ions?
Add one electron for each negative charge and subtract one electron for each positive charge
Which elements have empty d orbitals available to accept electrons?
Elements in the third row
What happens when two nonmetals combine or a metalloid bonds to a nonmetal?
A covalent bond is formed
What is a molecule?
A discrete group of atoms held together by covalent bonds
What is the main purpose of drawing a Lewis structure?
To show the location of all valence electrons in a molecule
What happens when a lone pair of electrons is converted into a bonding pair?
One bonding pair of electrons is formed for each 2 e− needed to complete an octet
What is the number of electrons that hydrogen shares?
2
What is the goal of atoms in forming covalent bonds?
To share electrons to attain the electronic configuration of the noble gas closest to them
Learn about covalent bonds resulting from electron sharing between atoms, molecules held together by covalent bonds, non-bonded electron pairs (lone pairs), and how atoms share electrons to achieve noble gas electron configuration. Explore the concept of covalent bonding in depth.
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