Ionic bonding Flashcards
Why do atoms bond
To increase their stability
Ionic bond
- Exchange electrons
- Look at the charges
- Electronegativity difference must be greater or equal to 1.7
Covalent bond
- Share electrons
- Look at prefixes
- Electronegativity difference is less than 1.7
Electronegativity def
- Gives a measure of how strongly an element will pull electrons to itself in a bond
- If there is not a large diff in electronegativity, electrons will be shared
- If there is a large diff in electronegativity, electrons will be exchanged
- Noble gases are out because they do not bond
How does ionic bodning work
- Metal atoms lose their valence electrons. This gives them a positive charge
- The nonmetals gain the electrons (adds to their valence). This gives them a negative charge. Nonmetals always have negative charges
- Ions are attracted to each other because of the charge
What is the size of an atom effected by
The attractive force of protons and repellive force of electrons
-As soon as you have net positive charge, electrons repell less, which means the protons can bring everything in and the ion gets smaller. The attraction between the electron and nucleus increases so ionization energy increases-> removing 2nd electron needs more energy than the 1st
Removing the 1st electron doubles, removing a third goes up because the first 2 were valence and the 3rd is making it a lot less stable. removing valence electrons increases the amount of energy because it is smaller, but once you get to breaking stability. Yjere will be a high jump of energy
What is ionization energy
-The amount of energy required to remove an electron
How would the size/radius of an atom affect ionization energy
As radius increases, ionization energy decreases (inverse)
How to tell how many valence electrons an atom has based on the ionization energy
-Look for the biggest jump in energy
How do you tell what element has the largest atomic radius based on the ionization energy
Look at the 1st ionization energy. The biggest radius has the smallest ionization energy. Larger ionization energy, so it is the smallest
What is coulombic attraction
The attraction between two particles of opposite charge
What two factors effect the strength of Coulombic attraction
- # of protons
- Distance between proton and electron
As you move across the periodic table (period), what factor is more important and how do you know
-# of proptons because distance doesn’t change much
As you move down the periodic table (group) which one of the factors is more important and how do you know
Distance because it increases and makes electrons easier to take even though number of protons increases
Electron affinity
The amount of energy given off when an atom get and electron
