ACP Chemistry Notes Chapter 7 Flashcards
Ionic bond
electrostatic attraction between closely packed, oppositely charged ions
- [metal cation]+ [non-metal anion]-
- the loosely held valence electrons of the metal atom easily reacts and has a high affinity for the non-metal atom; the electrons transfer between the metal and non-metal produce the ionic bond.
Oxidation
the metal transfers (loses) its valence electrons to the non-metal
Covalent Bond
a sharing of electrons by the nuclei of two non-metal atoms
- the valence electrons of two non-metals primarily reside in the space between two nuclei where they are attracted simultaneously by both protons, producing the covalent bond
Electronegativity
the amount of attraction an atom has for a valence shell electron of another atom; also related to the electron affinity = the amount of energy to add an electron to the valence shell of an atom (opposite to the ionization energy)
- electronegativity decreases going DOWN a group on the periodic table
- electronegativity increases going ACROSS a row on the periodic table
*Most electronegative element = F flourine
*Least electronegative element = Cs cesium
Where are the valence electrons located?
valence electrons are in the highest energy level and are in the outermost orbital or shell. Valence electrons are the farthest distance from the nucleus and have the weakest attraction for the positively charged protons in the nucleus of an atom
What does an atom’s electron configuration determine?
An atom’s electron configuration and valence electrons determine the chemical properties and reactivity of individual atoms and how they behave
What does an atom’s electron configuration tell?
The atom’s electron configuration explains its position and properties on the periodic table
Ionic bonding
Groups 1, 2, and 3 metals will lose electrons from their valence shell while groups 5, 6, and 7 non-metals will gain electrons from their valence shell to achieve noble gas configurations.
Covalent Bonding
Groups 4,5,6,7 will share valence electrons to allow both atoms to achieve noble-gas electron configurations
The octet rule
Elements will typically fill their valence orbitals with 8 electrons maximum; Stable compounds form when atoms achieve noble-gas electron configuration
Single bond
involves 2 atoms sharing 1 electron pair (2 e-). Ex. Group I,VII (hydrogen)
Double bond
involves 2 atoms sharing 2 electron pairs (4 e-) Ex. Group VI (oxygen)
triple bond
involves 2 atoms sharing 3 electron pairs (6 e-) Ex. Group V (nitrogen)
triple bond
involves 2 atoms sharing 3 electron pairs (6 e-) Ex. Group V (nitrogen)
Ion
Charged particle
