Bonding Flashcards
Ionic bonding
Transferring electrons between metal and non metal atoms
Covalent bonding
Sharing electrons between two non metal atoms
Metallic bonding
Share free electrons between two metal atoms
Compounds
Atoms which have formed bonds with each other by chemical reactions
Electrostatic attraction
The attraction between oppositely charged atoms
Ionic bonds
Electrostatic attraction between oppositely charged ions
Intermolecular forces
Weaker bonds between multiple atoms of the same molecule
Simple molecular structure
Covalent bonds between the same element
Giant covalent structure
Regular lattice made by covalently bonded atoms
Regular repeating lattices
The same formation of atoms repeated in a lattice form
Malleability
Ability to be bent / hammered into shapes
Ductile
Ability to be drawn into wires
Sonorous
Makes a sound when hit
Ion
Atom or group of atoms with an electric charge due to transferring electrons
Cations
Positive ions
Ations
Negative ions
S+
Slighty positive ion
S-
Slightly negative ion
Delocalised
Not in a fixed position
Graphine
A single layer of graphite
Allotropes
Different structural formations of the same element in the same physical state
Macromolecules
Giant covalent strucure
Alloy
A mixture containing one of more metal element
Properties of ionic compounds
- when solid, form white crystals and are not volatile
- very high melting and boiling point
- don’t conduct electricity unless moleten
- solids are soluble in water
- solids are insulators
Zn2+
Zinc (positive ionic compound)
Ag+
Silver - positive ionic compound
H+
Hydrogen- positive ionic compound
NH4+
Ammonium- positive ionic compound
Fe2+
Iron- positive ionic compound
OH-
Hydroxide- negative ionic compound
HCO3-
Hydrogen carbonate - negative ionic compound
What does ‘ide’ mean at the end of an ionic compound?
A simple compound made of two elements
What does ‘ate’ mean on the end of an ionic compound?
- another element often oxygen in involved
What are properties of simple molecular structures?
- easily change state
- volatile
- insulators
- conduct when dissolved in water
What does volatile mean?
- evaporates easily (has a strong smell usually)
What are the allotropes of carbon?
- diamond, graphite, nano tubes, fullerines
What are the properties of giant covalent structures? What are examples of giant covalent structures?
- very high melting points
- dont form molecules
- form regular repeating lattices
- all bonds are covalent (no intermolecular)
Examples include diamond, graphite and silicon dioxide
Properties of diamond
-very hard
- each carbon atom covalently bonded to 4 other carbon atoms
- doesn’t conduct
- giant covalent structure
Properties of silicon dioxide
- giant covalent structure
- made up of silicon and oxygen
Oxygen }2 silicon
Silicon}4 oxygen
In what type of structures are intermolecular forces ONLY used in?
Simple molecular
What are the properties for graphite
- composed of layers of graphine held together by weak intermolecular forces
- high melting point
- layers can slide off each other
What are the properties of graphine?
- hexagonal structure
- a single layer of graphite
- two delocalised electrons, so semi conductive
- transparent
- allotropes of carbon
What are the properties of nano tubes?
- stronger than steel (high tensile strength)
- rolled graphine
- good heat conductor
- unique electrical properties
What are the properties of Buckminster fullerene?
- can’t conduct
- 60 carbon atoms
- used as a solid lubricant (like microscopic ball bearings)
- each carbon atom bonded with 3 others (1=c-2)
- hollow football shape
What are the properties of metallic compounds?
- high melting point as strong attraction between positive charged ions and sea of electrons
- malleable
- ductile
- sonorous
- conduct
- strong and hard
- shiny
What is metallic bonding (process)
- all metals form positive ions when creating a full outer shell s all in centre of periodic table
- giant structures of positive ions create a regular lattice as they are packed tightly together
- outer electrons become delocalised and separate toform sea of electrons
- metal atoms become positively charged
- sea of electrons becomes negatively charged so becomes attracted to metal atoms
- sum of all electrons in the sea of electrons together make all the metal atoms have full shells
Why are metals so strong?
- metallic bonds don’t break as sea of electrons are free to move
Why are metals pure metals more malleable ?
- all metla atoms are same size and form layers
- when hit the layers can slide over each other rather than breaking
Why are alloys stronger than pure metals?
- alloys are made up if two or more different metals
- different metals have different size atoms
- when alloys form layered structure, the different sized atoms make the layered structure impossible and therefore the layers cannot slide over each other
