Ionic Bonding_Key Questions Flashcards
What is ionic bonding?
Ionic bonding is a type of chemical bondthat involves the electrostaticattraction between oppositely charged ions, and is the primary interaction occurring in ionic compounds.
What are Ionic Compounds?
Made by chemical combinations of metallic and non-metallic elements. Form a crystal lattice.
What is Crystal lace made up of?
Crystal lattice is made up of particles called cations and anions
How is Crystal lace held together?
The three dimensional lattice is held together strongly by electrostatic forces of attraction between the cations and anions
What are the 8 Properties of Ionic Compounds?
- have high melting and boiling points.
- are solids at room temperature.
- are hard but brittle.
- neither malleable nor ductile.
- do not conduct electricity in the solid state.
- are good conductors of electricity in the liquid state or when dissolved in water.
- have varying water solubility.
- not soluble in non polar solvents such as oil.
Explain the Properties of Compounds – generally:
- Forces between the particles are strong
- There are no free-moving electrons present as there are in metals
- there are charged particles present, but in a solid state are not free to move
- When an ionic compound melts, the charged particles are free to move and then the compound will conduct electricity
How does the ionic bonding model explain High Melting Point?
A large amount of energy is required to overcome the electrostatic attraction between the cations and anions in an ionic solid.
How does the ionic bonding model explain Hardness & Brittleness?
Hard –strong electrostatic forces between ions in an ionic compound makes that compound hard.
Brittle –disrupting the lattice will result in ‘like charges’ repelling each other and shattering the crystalline structure
How does the ionic bonding model explain Electrical Conductivity?
- For an object to conduct electricity, it must contain free-moving charged particles.
- solid ionic compounds do not contain free-moving ions, whereas melted (molten) or aqueous solutions of ionic compounds contain free moving particles that can conduct electricity.
How does the ionic bonding model explain Solubility?
- Some ionic compounds are very soluble, whilst some are not.
- The solubility of an ionic compound depends on the relative strength of the forces of attraction between: •Cations and anions in the lattice
•Water molecules and these charges particles (ions)
How are ionic compounds formed?
- metal atoms lose electrons to form positively charged ions (cations)
- Non metal atoms gain electrons to form negatively charged ions (anions)
- The ions present in an ionic compound have a stable electronic configuration identical to that of the noble gas nearest to them on the periodic table
- Electron transfer diagrams can be used to represent the formation of an ionic compound from its elements
- When formed from positively charged metal ions and negatively charged non-metal ions, the ions combine in proportions that produce an ionic compound with an overall zero charge
Explain why the crystal lattice is held together so strongly in sodium chloride even though the number of cations is equal to the number of anions.
The negative ions are slightly further away from each other than they are from the positive ions in the lattice and the attractive force of the oppositely charged ions outweighs the repulsive force of two positively charged or two negatively charged ions near each other.
Determine if the Substance is likely to be an ionic compound. Substance A has a melting point of 842 degrees and conducts electricity at 700 degrees.
No
Determine if the Substance is likely to be an ionic compound. Substance B has a melting point of 308 degrees and It does not conduct electricity at 250 degrees but will conduct electricity at 350 degrees
Yes
