Test 6 Flashcards
what are good examples of atoms with stable electron configurations
noble gases
bonding usually __ energy as the atom’s electron configurations attain lower energy states
releases
why do atoms with more than 4 valence electrons tend to gain electrons?
they have relatively high electron affinities
__ is the tendency of an object to form 2 localized regions of opposite character
polarity
can a completely ionic bond result from electron transfer? why? why not?
no, that would imply that the donor atom had no affinity for the donated electrons
what is a bonding pair of electrons and where are they found?
the two shared electrons that make up a pair. they are in between the nuclei
what is electrostatic force
the force exerted between electrical charges
name the natural diatomic elements
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine
when using Lewis structures, a __ is substituted for the bonding pair to simplify the diagram
dash
in a Lewis structure a dash represents how many electrons?
2
The element with the most __ electrons will likely be the central atom
bonding sites/unpaired electrons
most polyatomic ions are __, formed by acquiring additional electrons to make up their octet
anions
how many atoms can hydrogen have
2
what is the hardest natural substance known?
diamond
the melting points of ionic compounds are at least__, illustrating just how __ their bonds are. describe ionic compounds
800*C
strong
dense, brittle, and hard solids
An __ is a mixture of a metal’s atoms with another element and has metallic properties
alloy
what kind of energy moves quickly through metallic objects
thermal
the shape of a metal object can be changed by hammering or stretching __ significantly affecting its __
without
strength
covalent bonds
Two atoms held together by their mutual attraction for the same pair of electrons. It usu- ally involves two nonmetals
ionic bonds
The attraction and electron transfer between two oppositely charged ions in a solid. It usually involves a metal and a nonmetal.
metallic bonds
A communal sharing of electrons between metal atoms.
A force of attraction produced by transferring or sharing electrons that holds atoms together in compounds.
chemical bonds
states that an atom tends to gain, lose, or share electrons until its outer level s and p orbitals are filled with eight electrons. This activity gives an element the electron configuration and stability of a noble gas.
octet rule
in covalent bonding…
electrons are shared
CNN
covalent nonmetal nonmetal
IMN
ionic metal nonmetal
MMM
metallic metal metal
guidelines for creating Lewis structures
- Lewis structures illustrate only compounds consisting of covalent bonds.
- Electron sharing occurs when one nonmetal atom bonds with another (e.g., hydrogen and fluorine) or when two identical nonmetal atoms bond (e.g., fluorine and fluorine).
- Each nonmetal generally forms covalent bonds to achieve eight electrons in its valence shell, including bonding and nonbonding electrons. Hydrogen is a major exception since its valence shell holds only two electrons.
- Electrons are normally shared in pairs since two electrons of opposite spin occupy empty orbitals.
- Polyatomic molecules, which contain three or more atoms, have one or more central atoms bonded to surrounding atoms. Since hydrogen can share only one pair of electrons, it can never be the central atom in a polyatomic molecule. Atoms with valence structures similar to Group 14 atoms (the carbon family) are more likely to be the central atom in a polyatomic molecule.
- The number of valence electrons for nonmetals (except hydrogen) can be predicted by the formula valence e– = group number – 10. The number of covalent bonds in which nonmetals can participate is predicted by the formula covalent bonds = 8 – valence e–
A group of atoms that maintains a constant electrical charge while existing as a unit in a wide variety of chemical reactions
polyatomic ion
An extensive three-dimensional structure that represents the regular pattern of atoms or ions
crystal lattice
A theory that offers an explanation of how metals bond: the valence electrons of atoms are said to be freely shared among all atoms
electron sea theory–associated with metallic bonds
An electron that can move between several different bonds
delocalized electron
why do electrons rearrange during bonding?
to maximize stability
