Molecular Shapes and Bond Angles in Chemistry

Electron pairs repel and try to get as far apart as possible to a position of minimum ______.

If there are no lone pairs, electron pairs repel ______.

Lone pairs of electrons repel more than bonding pairs due to ______.

Lone pairs reduce bond angles by about 2.5 degrees per lone pair to minimize ______.

Square planar shape has a bond angle of ______ degrees.

Linear shape has a bond angle of ______ degrees.

A compound with elements of similar electronegativity will have a _______ bond

A compound with elements of very different electronegativity will have an _______ bond

In a polar compound, the element with the larger electronegativity will be the δ- _______

A polar covalent bond forms when the elements have different electronegativities between _______ to 1.7

A symmetrical molecule with all identical bonds and no lone pairs will be _______

CO2 is a symmetrical molecule and considered a _______ molecule

The strong electrostatic forces between positive ions and a sea of delocalised electrons require a lot of energy to break due to high _____________.

Solubility in water is generally good for substances that form _____________.

Conductivity when solid is generally poor because the ions are fixed in the lattice and cannot _____________.

Diamond and sand exhibit poor conductivity because electrons are _____________.

Malleability in shiny metals is due to the identical positive ions in the lattice, allowing planes of ions to easily _____________.

The shape of a molecule is determined by the number of bonding pairs and lone pairs of _____________.