Chem 20 ch. 3: Understanding Chemical Compounds

This formula shows the way in which atoms are bonded to each other.

Answer explanation

The development of this started with Frankland, who stated that each element has a fixed bonding capacity.

Then, Kekule extended the idea to illustrating a bond as a dash between bonding atoms.

A ________ results from the simultaneous attraction of electrons by 2 atomic nuclei.

Answer explanation

The explanation for bonds in the diagrams started with Abegg.

He first suggested that bonding capacity must be associated with an atom's electron structure.

Then, he suggested that the stability of the noble gases was due to the amount of electrons in the atom.

EX: A Na atom needs one more electron for stability.

Na + Cl yields

Na+ + Cl- yields

NaCl.

This is a specific area of space where there is a high chance of finding electrons of particular energy.

Answer explanation

Valence orbitals are the same definition but are in the highest energy level.

They contain 1, 2, or no electrons.

True or False: Electrons "spread out" to occupy any empty valence orbitals before forming electron pairs. For example, 6e- leads to 2e-, 2e-, 1e-, 1e-.

• True

• False

True or False: Electrons "spread out" to occupy any empty valence orbitals before forming electron pairs.

EX: 6e- (arrow) 2e-, 2e-, 1e-, 1e-.

8e-

2e-

16p+

S
Sulfur atom

• True

• False

This is the ability for an atom to attract electrons to itself when chemically combined with another element.

Answer explanation

Metals tend to have low electronegativities. Nonmetals have high electronegativities.

EX: Chlorine's electrons are strongly connected to the nucleus because the atom is small. Lithium's electrons aren't strongly connected to the nucleus because the atom is big. SOOOO, lithium loses the electron tug of war because chlorine has the ability to attract its electron.

(Seperate your answers with a space)

On the periodic table... as the electronegativity increases, the size of the atom (increases/decreases). As the electronegativity decreases, the size of the atom (increases/decreases).

-non metal + non metal

-the simultaneous attraction of 2 nuclei for a shared pair of bonding electrons

-if the electronegativities of both atoms are high, neither atom will "win" and the pair of bonding electrons will be shared instead.

• Ionic bond

• Covalent bond

• Chemical bond

• Metallic bond

Answer explanation

Electron sharing between atoms with high electronegativities results in covalent bonding.

-metal + non metal

-if the electronegativities of 2 colliding atoms are different, the atom with the stronger attraction for electrons may succeed in removing that bonding electron from another atom.

-positive and negative ions are formed

-Arranged in a 3-dimensional crystal lattice structure

-Each + ion is surrounded by - ions and vice versa

• Chemical bond

• Metallic bond

• Covalent bond

• Ionic bond

Answer explanation

If the competing atoms have unequal electronegativities, the result may be unequal covalent bonding since an electron transfer occurs.

-Metal + metal

-If the electronegativities of 2 colliding atoms are low, the atoms share valence electrons.

-No actual chemical reaction takes place

-Pure metals have closely packed cations suspended in a 'sea' of free electrons that move between the cations.

-The valence electrons aren't held strongly by their atoms

-Have vacant valence orbitals

-The valence electrons act as a glue holding the whole structure together.

• Covalent bond

• Ionic bond

• Metallic bond

• Chemical bond

Answer explanation

Fun fact: the free electrons transmit kinetic energy quickly, so that explains why metals are excellent conductors of heat.

The free electrons move quickly in response to an electric field.