Bonding

• What is ionic bonding?

  transfer of electrons between atoms ; nonmetal X metal
• What is covalent bonding?

  sharing of electrons between atoms ; nonmetal X nonmetal
• What is metallic bonding?

  electrostatic attraction between positively charged metal ions and a sea of delocalized electrons ; metal X metal
• How can an element become stable?

  filling the outer electron shell
• What is the definition of malleable?

  shape/hit into an object
• What is the definition of ductile?

  stretch into a shape
• What is the definition of aqueous?

  containing water
• What is ionic bonding caused by?

  electrostatic attraction between oppositely charged ions
• What happens if the number of electrons increase?

  electrical conductivity increases
• Why do melting points increase when going up the periodic table?

  more shielding - strong force of attraction between metal ions and delocalised electrons require higher energy to break
• Why can metals conduct electricity?

  delocalised electrons - free to move around and transfer electrical charge
• Why can metals be shaped into objects without shattering?

  metals are in layers - can slide over each other meaning can change shape while still maintaining their metallic structure
• What are the characteristics of covalent bond?

  lower melting point & low electrical conductivity
• What does covalent bonded element exist as in room temperature?

  usually as liquid or gas
• Are covalent bonds soluble?

  insoluble in water & soluble in organic solvent
• How strong is the intermolecular forces between covalent bonds?

  relatively weak
• What is a dative/coordinate bond?

  an atom provides both electrons
• What must the acceptor atom be in dative/coordinate bond?

  electron deficient
• Do giant ionic lattice have a high or low melting point, why do they have these melting points?

  high - strong electrostatic forces take a great deal of energy to separate positive and negative ions in a crystal lattice
• Can ionic compounds conduct electricity and what is the explanation?

  yes - when molten ions are able to move in a liquid state allow to transfer charge & no - unable to conduct when solid
• Why do ionic compounds shatter easily?

  lattice is made of alternative positive and negative ions
• What is occurring during an ionic compound shattering?

  ions with the same charge are forced to repel causing shatter
• How are giant lattice structures , eg metals, held together?

  strong electrostatic forces between positive ions and free electrons
• What are the features of strength considered for metallic bonds?

  number of protons & number of electrons & size of ion
• If a potential difference is applied to a metal, what happens?

  free electrons move away from the negative terminal due to repulsion & free electrons are attracted towards the positive terminal due to attraction
• What is a lone pair?

  atom donating electron
• What is the definition of electronegativity?

  ability of an atom to attract a pair of electrons in a covalent bond
• What is electron density?

  way negative charge is distributed in a molecule
• What does electronegativity depend on?

  nuclear charge & atomic size & distance between nucleus
• What is the definition of non-polar?

  equal sharing of electrons
• What is the definition of polar?

  electrons are not shared
• What type of force is stronger, intermolecular or intramolecular?

  intramolecular
• What are the three types of intermolecular forces, from weakest to strongest?

  van der Waals & dipole-dipole & hydrogen
• What element has the strongest electronegativity?

  fluorine
• What are the characteristics of Van Der Waals?

  non-polar molecules & weak
• Are Van Der Waal forces in all molecules?

  yes
• What are characteristics of Dipole-Dipole forces?

  permanent & polar molecules
• What are characteristics of Hydrogen forces?

  strong & has hydrogen
• What are the only elements that can bond to hydrogen and form Hydrogen bonding?

  fluorine & oxygen & nitrogen
• What is the definition of Hydrogen bonding?

  attraction between a lone pair of electrons and electron deficient hydrogen atom