Chemical bonds Flashcards
covalent bond
Type of bond made with two or more nonmetals that equally share electrons, no electron movement, no charge
ionic bond
Type of bond made between a (low IE) metal and a (high EN) nonmetal, complete transfer of electrons, +/- charge
metallic bond
Type of bond made between metals
polar covalent bond
Type of bond made between two or more nonmetals that unequally share electrons creating small charges, shifts electrons closer to the atom, partial (+) and partial (-)
An atom that loses an electron becomes a
Positive ion
Nonmetals
gain electrons becoming negative
Metals have
low ionization energy causing them to lose electrons
A/An __________ is an ion with a negative (-) charge.
anion
Metals __________ electrons to form _____________
lose; cations
In an ionic bond, oxygen forms what charge?
2-
What types of atoms make up a covalent bond?
nonmetal + nonmetal
What happens to the electrons in a covalent bond?
they are shared between atoms
Which is true about the atoms in a covalent bond?
they both have high ionization energy and high electronegativity
Diatomic molecules are atoms that covalently bond to themselves. Which of the following are diatomic molecules in nature?
F, N, O, I, Cl, Br, H
How many electrons are shared in a double bond?
2
Ionic Compounds
High melting and boiling points, Soluble in water, and
Conduct electricity when dissolved or melted
Covalent Compounds
Tend to be gases, liquids, low-melting solids and weak intermolecular forces
How many valence electrons do most elements need in order to be stable?
8
How many electrons does Hydrogen need to become stable?
2
Magic Number of electrons
same as noble gases because of stability
Octet Rule
elements are stable with 8 valence electrons, only applies to things with 8 electrons
Duet Rule
elements stable with 2 valence electrons, very small atoms (H, He, Li, Be, B)
chemical bond
attractive forces that hold atoms together, formed by valence electrons, no charge
non-polar covalent range
0.0-0.2, no shift in electrons
polar covalent range
0.3-2.0, electrons closer to one atom, partial charges
ionic bond range
2.0-4.0, electrons are transferred from one atom to another, complete charges
ionization energy left side
low IE, easy to take electrons, metals, electronegativity: low EN, not going to take electrons
ionization energy right side
non-metals, high IE, doesn’t lose electrons, electronegativity: high EN, strong pull on other electrons
noble gases
most stable, full of valence shells, has stability
ionic
transfers electrons, +/- charge, low IE, high EN, metal + non-metal
covalent
shares electrons, no charge, high IE and EN, non-metal + non-metal
hydrogen rule
never in the center, has non dots, and only needs one bond
polyatomic
don’t always follow expected number bonds, sometimes need 1 double bond but multiple options to put it
lone pairs
Valence electrons that are not involved in covalent bond formation
single bonds
two atoms held together by one electron pair
double bond
two atoms share two pairs of electrons
multiple bond
two atoms share two or more pairs of electrons
triple bond
two atoms share three pairs of electrons
valence shell
The outermost electron occupied shell of an atom, which holds the electrons that are usually involved in bonding.
