Metallic Bonds
What are 2 properties of metals?
Malleable
Ductile
Good conductors
Shiny
What type of elements form ionic bonds
metal non metal
What is true of stability and Ep when a bond forms?
Stability high
Ep low
What causes metals to be malleable
Their bonding structure is such that the "sea of electrons" and cations are not fixed in position. They particles can move (when you bend them) and still maintain attractions
Where are metals found on the periodic table?
Left hand side and middle
2 nuclei simulataneously attracting each others valence electrons
very different
metal low
non metal high
When two atoms are very far apart, what is true of the potential energy of the system
It is relatively high
Why is an anion larger than its neutral atom?
additional e causes increased repulsion
What makes metals good conductors?
They have delocalized electrons that are not strongly attracted to the cations and these electrons can move when a potential difference (or charge difference) is applied
non polar covalent
What causes the metal to give up its electron?
Has a low ionization energy
What factors are important in determining the potential energy of a system of charged particles
charge and distance
What types of bonds can fundamentally be described as forces of attraction
Describe the structure of a metallic bond
Cations surrounded by a "sea of electrons" or delocalized electrons
If the electronegativities of the atoms involved in the bond are high but unequal, what type of bond forms?
polar covalent
What causes the non metal to attract the electron
High effective nuclear charge and/or high attraction for electrons, high EN
If attraction is very strong between particles or you have a "strong bond", what is true of the Ep of the system
It is very low
Why is share a bad word to describe a covalent bond? What is a better term to use?
Tug of war is a better analogy
What do delocalized electrons mean?
Electrons that are not associated with only 1 or 2 atoms /ions, but are attracted by several atoms/ions
What is a triple bond
2 nuclei simultaneously attract 6 electrons
What causes the ionic crystal lattice structure?
Ions pack so as to maximize attraction and minimize repulsion, thereby increasing stability and decreasing potential energy
What is the bond energy and bond length?
BE - energy input required to break the bond
BL- internuclear distance between atoms in bond
What causes the high melting point of NaCl?
Strong attraction between ions