Chemistry, Inter- and Intra-Molecular Bonds... and Lewis Diagrams!

Going down the halogens, INTER-molecular London Dispersion Forces goes up because:

A requirement of dipole-dipole interactions and hydrogen bonding is:

HClO4 is a rocket fuel. An O-Cl bond is best described as:

Ethyne Lewis structure is:

Dipole-dipole intermolecular forces:

Pure I₂ is a solid at room temperature whereas F₂ is a gas at room temperature because:

London Dispersion Forces are important in:

Which has a higher boiling temp, CBr₄ or CCl₄?

ICl or Br₂: which has a higher boiling temp, and why?!

BCl₃: Which is true of B?

"Not... For... Ourselves"... this acronym can be used to remember N, F and O...three atoms that:

If O and H atoms share a bond, the bond is BEST described as:

The attraction between HF and HF is an example of what kind of intermolecular force?

Why does the rubber of a balloon (containing water) not melt when a flame is placed under it?

Going down the halogen family, the strength of intra-m. covalent bonds b// identical atoms:

Generally, intramolecular bonds are stronger than intermolecular bonds.

In general, when an atoms forms an ion, the atoms loses/gains e-s to attain:

To determine the chemical formula for an IONIC compound:

Ionic bonds are very strong. Therefore, compounds held together with ionic bounds:

When drawing a Lewis diagram for an individual atom, we draw 4 orbitals. UN-paired electrons:

Lewis Dot structures should include...

There are two types of Van der Waals bonds, intermolecular and intramolecular

In Ethyne, C is more electronegative than H. This results in:

According to Hebden, molecules must be ______ ______ in order to be polar:

It turns out Al, H, Be and B ("Al Has Been Busy") do not follow the octet rule. We know that:

If we had multiple acetone molecules in nail polish, we would expect to have:

Most ionic bonds are stronger than most dipole-dipole bonds

Polar covalent compounds generate dipole dipole attraction

Lewis dot structure is all about protons?

Covalent bonds are super strong. You would therefore expect them to have:

Column 17 elements have how many valence electrons in total?

F atom meets F atom and forms:

PH_{3 or} NH₃: which has a higher melting temp, and why?

Atoms that are more electronegative are generally less polarizable because:

BCl₃: how many bonding electrons, in total?

Water molecules are capable of the most important intermolecular bonds:

BCl₃: polar or non-polar, and why?

L.D.F.s are only significant when no ionic or dipole-dipole inter-molecular bonds form because:

More shared or bonding electrons between two atoms results in:

Neutral, column 17 atoms have:

Column 14 elements of the carbon group tend to have a VALENCE of:

Lewis dot structure are a useful tool to predict existence of lone pair

Who created Lewis Dot Structures?

Covalent bonds form between:

If He atoms move slowly enough at super low temps, L.D.F.s allow for this phase transition:

Sulfur has:

P and Cl will form a:

Column 13 elements, Boron and Aluminum, must be:

Why are hydrogen bonds a relatively strong inter-molecular bond?

If you were to melt solid O₂ (as depicted below) which bonds would break first?

Which is true when drawing Lewis Structures?

Less than a full valence shell is sometimes called:

BCl₃... how many lone-pair electrons in total?

The octet rule, in terms of covalent bonding, helps to remind us that:

In an ionic bond:

Difference between dipole-dipole and ionic bonds:

Will the molecule be polar or non-polar? Hint: look for electronegativities, and think symmetry

Why are small atoms like Helium not easily polarized?

Polarizability is a funny concept. Which is true?

Solve this rebus puzzle:

Electron-dot diagrams are also called Lewis diagrams. They show:

Non-polar covalent compounds generate dispersion forces

London Dispersion Forces increase going down a column because:

What do Lewis Dot Structures show?

Going across a row, electronegativity increases BUT L.D.F.'s increase because: