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Period properties & bonding assessment
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1) As we move from left to right in a period, ionization energy increases. Ionization energy isdecided based on the distance of nucleus and electrons, since sulfur is higher than phosphorus,
ionization energy is also higher.
2 2 6 2 3
2) The electron configuration of phosphorus is 1𝑠 2𝑠 2𝑝 3𝑠 3𝑝 and the electron configuration
2 2 6 2 4
of sulfur is 1𝑠 2𝑠 2𝑝 3𝑠 3𝑝 . P can hold up to 6 electrons and each box needs to have 2
electrons. Sulphur has 4 electrons in 2 boxes making it stable. Phosphorus has 3 electrons
making it unstable and rushing to find an electron and make itself stable again. This property
makes sulfur less in ionization energy than phosphorus.
3) As we go down the halogen group, more orbitals are added until the electrons in the element
match the same number as the atomic number. The farther the electron is from the nucleus, the
harder it is to accept electrons and make bonds.
4) In a metallic bond both the first and second atom have low electronegativity and ionization
energy. In ionic bonds the first atom has low electronegativity and ionization energy, the second
atom has high electronegativity and ionization energy. In covalent bonds, both atoms have high
electronegativity and ionization energy. In metallic bonds since both atoms have the same
properties, they will bond with each other and other metals. In ionic bonds one atom is low and
the other is high, we know that unlike charges attract. In covalent bonds both atoms have the
same properties and they will bond together.
5) Electronegativity values
6) H-H, S-H, CL-H, O-H, F-H.
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