Chemical Bonding
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What is a chemical bond?
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds.
What are the three main types of chemical bonds?
Ionic bonds, covalent bonds, and metallic bonds.
Define ionic bond.
An ionic bond is a type of chemical bond formed through the electrostatic attraction between oppositely charged ions.
What typically forms ionic bonds?
Ionic bonds typically form between metals and nonmetals.
Define covalent bond.
A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms.
What is a characteristic property of metallic bonds?
They allow metals to conduct electricity and heat.
What is atomic size?
Atomic size refers to the distance from the nucleus of an atom to the outermost shell of electrons.
How does atomic size change across a period in the periodic table?
Atomic size decreases from left to right across a period.
How does atomic size change down a group in the periodic table?
Atomic size increases down a group.
What is the trend of ionization energy as atomic size increases?
Ionization energy decreases as atomic size increases.
Define electronegativity.
Electronegativity is the ability of an atom to attract electrons in a chemical bond.
What type of bond is likely to form between atoms with high electronegativity differences?
Ionic bonds are likely to form.
What is a polar covalent bond?
A polar covalent bond is a type of covalent bond where electrons are shared unequally between atoms.
What is the octet rule?
The octet rule states that atoms tend to bond in such a way that they have eight electrons in their valence shell.
Define lattice energy.
Lattice energy is the energy released when ions bond to form an ionic solid.
How does lattice energy relate to ionic bond strength?
Higher lattice energy indicates a stronger ionic bond.
What is the role of valence electrons in bonding?
Valence electrons are the electrons involved in forming bonds between atoms.
What is meant by ‘bond polarity’?
Bond polarity refers to the distribution of electrical charge over the atoms in a bond.
What determines whether a bond is ionic or covalent?
The difference in electronegativity between the bonded atoms determines if a bond is ionic or covalent.
Name 3 factors that show that a bond is most likely ionic
• Ionization energy 2.Electron Affinity • Lattice Energy
Why does atomic radius decrease across a period?
Across a period, nuclear charge increases as more protons are added. Electrons are added to the same energy level, so shielding remains constant. The increased nuclear attraction pulls the electrons closer to the nucleus, decreasing atomic radius.
What are the hypothetical steps in the formation of NaCl(s) from elements in their standard states?
Sublimation of Na(s)→Na(g) First ionisation energy of Na(g)→Na(g) + e Bond dissociation energy Cl₂→Cl Electron affinity of Cl + e →Cl‾ Lattice formation (Na⁺ + Cl⁻ → NaCl(s))
What are the hypothetical steps of the formation of MgO
Sublimation of Mg(s)→Mg (g) First ionisation energy of Mg (g)→ Mg +e Second ionisation energy of Mg (g)→ Mg (g) +2e Bond dissociation energy ½O₂(g) → O(g) First electron affinity O(g) + e⁻ → O⁻(g) Second electron affinity O⁻(g) + e⁻ → O²⁻(g) Lattice energy Mg²⁺(g) + O²⁻(g) → MgO(s)
Why is the second electron affinity of oxygen endothermic in the formation of MgO?
The second electron is added to an already negative ion (O⁻), so energy is needed to overcome electrostatic repulsion