periodicity, Ionisation Energy, And Electronegativity Flashcards
what are the elements in the periodic table ordered by ?
increasing atomic size
what happens to the number of shells going down a group ?
increases
what happens to the number of shells going along a period ?
stays the same
what happens to the number of outer electrons going down a group ?
stays the same
what happens to the number of outer electrons going along a period ?
increases
what happens to the first ionisation energy going along a period ?
increases
what happens to the first ionisation energy down a group ?
decreases
what happens to charge going along a period ?
increases
what type of bonding is present in H2
covalent molecular
what type of bonding is present in Li
metallic lattice
what atoms are monatomic
Noble gases (group 0)
what type of bonding is present in O2
covalent molecular
what type of bonding is present in s8
covalent molecular
what type of bonding is present in C60
covalent molecular
what elements are covalent networks
B, C (diamonds and graphite), and Si
explain metallic bonding
the attraction between a sea of delocalised, negatively charged electrons and positively charged metal ions.
the force of attraction between them causes metallic bonds
Explain covalent molecular bonding
The covalent bond is formed by a shared pair of negative electrons electeostatically attracted to the positively charged nucleus between 2 non metal atoms.
Explain monatomic bond
Single atoms containing a full outer shell of electrons
What is the first ionisation energy ?
The energy required to remove one mole of electrons from a gaseous atom
What is the second ionisation energy ?
The energy required to remove a second mole
Why does the ionisation energy increase across a period
As the nuclear charge increases the pull of the nucleus on the electrons increases. Meaning the electrons are closer to the nucleus and therefore require more energy to remove
Why does the ionisation energy decrease down a group ?
As more shells are added the inner electrons shield the outer electrons from the pull of the nucleus.
Therefore making it easier to remove electrons
Why does the electronegativity increase across a period ?
The electronegativity increases because the nuclear charge increases (the higher the positive charge, the stronger the pull for negative electrons)
Why does the electronegativity decrease down a group ?
The electronegativity decrease because of inner electrons shielding outer electrons
