Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
26 Cards in this Set
- Front
- Back
What are the terms bond length and bond angle?
|
Bond length - Distance between the nuclei of 2 bonded atoms
Bond angle - Angle between two covalent bonds |
|
What is the bond angle of a tetrahedral?
|
107.5 degrees
|
|
What is the electron pair repulsion theory?
|
Lone Pair - Lone Pair repels more then Lone Pair - Bond Pair repels more than Bond Pair - Bond Pair.
LP-LP > LP-BP > BP-BP |
|
How many lone pairs and bond pairs are in a pyramidal shaped molecule?
|
3 Bond Pairs
1 Lone Pairs e.g. NH3 |
|
What is the name given to this term?
'Different forms of the same element in the same physical state' |
Allotropes
|
|
What makes Diamond different to Graphite? (3 differences)
|
1.The Carbon in Diamond has 4 bonded electrons where as in Graphite it has 3 bonded electrons.
2.Due to the bonding Diamond doesn't conduct electricity where as Graphite does. 3.Graphite has weak intermolecular forces between layers where as Diamond doesn't due it's rigid structure. |
|
What is electronegativity?
|
a measure of the tendency of a atom a covalent bond to attract other bonding electrons
|
|
Why does electro-negativity increase along a period?
|
Atomic radius decreases so outer electrons are more attracted to the nucleus.
No. of protons in nucleus increases so greater puller on electrons. |
|
Why does electro-negativity decrease down a group?
|
Atomic radius increases so outer electrons are far away from the nucleus therefore less attracted
|
|
What character will a molecule resemble when the electro-negative difference is large and when the difference is small?
|
Large electronegative difference = Ionic character
Small electro-negative difference = Covalent character |
|
When do polar bonds exist?
|
When there's a difference in electro-negativity between 2 atoms
|
|
What does a positive and negative dipoles indicate about electro-negativity in a molecule?
|
Positive dipole - atom is slightly positive
Negative dipole - atom is slightly negative Electro-negativity - Negative dipole > Positive dipole |
|
Why do noble gases have on electro-negative value?
|
They have full outer shells therefore wouldn't have a tendency to attract other atoms
|
|
What properties do polar molecules share?
|
1.Different bonds
2.Identical bonds and lone electron pairs on central atom 3.Asymmetrical |
|
What do non-polar molecules share?
|
1.Symmetrical
2.Same bonds 3.No lone pairs |
|
What does the term intramolecular mean?
|
Bonding within a molecule e.g. ionic, covalent bonding
|
|
What does the term intermolecular mean?
|
Forces of attraction between molecules, they determine melting and boiling points. e.g. London forces and hydrogen bonds
|
|
What are the 3 main intermolecular forces?
|
1.Hydrogen bonds (strongest)
2.Permanent dipole-dipole attraction 3.London forces (weakest) |
|
What are London forces also known as?
|
Van Der Waals forces
|
|
What are London forces?
|
Intermolecular forces that exist between molecules. They arise from temporary attraction between neighbouring dipoles.
|
|
Which of the 3 main intermolecular forces is the strongest?
|
Hydrogen bonds
|
|
Why is ice less dense than water?
|
The hydrogen bonds in solid ice holds the molecules further apart than in a liquid
|
|
What type of bond holds the double-helix in DNA (deoxyribonucleic)?
|
Hydrogen bonds between base pairs
|
|
What property does a substance have if it can form hydrogen bonds with water?
|
Becomes more soluble e.g. ethanol
|
|
What bond does HF form (hydrides)?
|
Hydrogen bonds
|
|
What bond develops when a molecule has many electrons?
|
Strong London forces
|