Chemistry: 1.3 Bonding Part 1
This flashcard set describes the nature of metallic bonding, highlighting the attraction between delocalised electrons and positive metal ions. It also explains the regular arrangement of metal ions and the role of mobile electrons in giving metals their characteristic properties.
Metallic bonding
The attraction between delocalised outer shell electrons and positive metal ions in a lattice
Key Terms
Metallic bonding
The attraction between delocalised outer shell electrons and positive metal ions in a lattice
How are the metal ions arranged
Packed close together in layers in a regular way
What are the metal ions surrounded by
Mobile electrons
What do mobile electrons do
Move freely within structure
What does delocalised mean
Displaced from where it’s expected to be
What does giant mean
A huge structure- consisting of millions and millions of atoms
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| Term | Definition |
|---|---|
Metallic bonding | The attraction between delocalised outer shell electrons and positive metal ions in a lattice |
How are the metal ions arranged | Packed close together in layers in a regular way |
What are the metal ions surrounded by | Mobile electrons |
What do mobile electrons do | Move freely within structure |
What does delocalised mean | Displaced from where it’s expected to be |
What does giant mean | A huge structure- consisting of millions and millions of atoms |
What does the number of delocalised electrons depend on | How many electrons are lost from each metal atom |
What is ionic bonding | The electrostatic attraction between oppositely charged ions in a lattice |
Where does ionic bonding occur | Between metals and non metals |
What happens in ionic bonding | Electrons are transferred from a metal to a non metal |
What is formed as a result of ionic bonding | Positive and negative ions |
What do metal atoms do | Lose electrons and become positively charged |
What do non metals do | Gain electrons and become negatively charged |
What is the charge on a simple ion related to |
|
What ion is formed from group 1 elements | +1 |
What ion is formed from group 2 elements |
|
What ion is formed from group 3 elements | +3 |
What ion is formed from group 5 elements | -3 |
What ion is formed from group 6 elements | -2 |
What ion is formed from group 7 elements | -1 |
What does boron not do | Form ions (covalently bonds) |
What can transition elements do | Form more than one stable ion |
What are compound ions | Covalently bonded species carrying a charge Eg. Hydroxide and carbonate |
Covalent bond | Shared pair of electrons |
Where does covalent bonding occur | Between atoms of non- metals |
What is a pair of electrons which is not bonded called | A lone pair |
When is a double bond formed | When 2 pairs of electrons are shared |
When is a triple bond formed | When 3 pairs of electrons are shared |
What is a non- octet molecule | A molecule where the central atom doesn't have a noble gas electron arrangement (8 electrons in a full shell) |
Coordinate/dative bonding | A covalent bond in which both electrons of the shared pair come from the same atom |
The atom that donates the electrons has a… | Lone pair |
The atom that accepts the electron pair does not have a full outer shell of electrons. It is… | Electron deficient |
How can coordinate bonds be shown | Using an arrow. The arrow points from the atom donating the electrons |
What happens once the coordinate bond is formed | It behaves like a normal covalent bond |
What 3 things is the shape of a molecule determined by | The total number of electron pairs around the central atom The number of bonding pairs of electrons The number of lone pairs of electrons |
What can the shape of molecules be predicted by | The electron pair repulsion theory |
What does the electron pair repulsion theory state |
|
How to draw a bond in the plain of the paper | A line |
How to draw a bond coming out of the paper | A wedge |
How to draw a bond going into the paper | A dotted line |
What are compound ions | Covalently bonded species carrying a charge |
What shape is a molecule with 2 bond pairs and no lone pairs | Linear |
What is the bond angle of a linear structure | 180 |
What is the shape of a molecule with 3 bond pairs and 0 lone pairs | Trigonal planar |
What is the bond angle of a trigonal planar | 120 |
What is the name of the molecule with 4 bond pairs and 0 lone pairs | Tetrahedral |
What is the bond angle of a tetrahedral structure | 109.5 |
What shape is the molecule with 5 bond pairs and 0 lone pairs | Trigonal bipyramidal |
What are the bond angles for a trigonal bipyramidal structure | 90 and 120 |
What is the shape of a molecule with 6 bond pairs and no lone pairs | Octahedral |
What is the bond angle for an octahedral structure | 90 |
What is the bond angle in an octahedral structure | 90 |
Do bonding pairs of electrons in double/triple bonds repel in the same way | Yes so the shape and bond angle are the same |
What is the shape of a molecule with 2 bond pairs and 1 lone pairs | Bent v-shaped |
What is the bond angle of a bent v shaped molecule with 1 lone pair | 118 |
What is the shape of the molecule with 3 bond pairs and 1 lone pair | Pyramidal |
What is the bond angle of a pyramidal structure | 107 |
What is the shape of the molecule with 2 bond pairs and 2 lone pairs | V shaped |
What is the bond angle of a v shaped molecule with 2 lone pairs | 104.5 |
Why is the bond angle smaller for a v shaped molecule with 2 lone pairs than a v shaped molecule with 1 lone pair | More repulsion |
What is the shape of a molecule with 3 bond pairs and 2 lone pairs | Trigonal planar |
What is the bond angle of a trigonal planar | 120 |
What is the shape of a molecule with 4 bond pairs and 2 lone pairs | Square planar |
What is the bond angle in a square planar | 90 |
What happens when an atom forms a coordinate bond | The shape changes as the number of bonding and lone pairs change |
Why does the shape of a molecule change when a coordinate bond forms | Bond pairs repel less than lone pairs so bond angle increases slightly |