bonding Flashcards
what is an ionic bond?
when will you primarily see them between elements?
- an electrostatic attraction between oppositely charged ions
- between elements with a big difference in electronegativity OR CHARGE DENSITY
what type of structures are formed as a result of an ionic bond “_____ _____ _____”
what are the ions in a giant ionic lattice held by?
why is an ionic compound a solid at room temperature?
why do ionic compounds conduct when molten or aq?
why can’t ionic compounds conduct when they are a solid?
- giant ionic structures
- strong electrostatic forces of attraction that HAPPEN in all directions
- the strong electrostatic forces of attraction require huge amounts of energy to overcome
- the ions ARE FREE to move and carry a charge
- the ions cannot move apart from each other
how does covalent character occur?
tell me 3 instances where a covalent character is most likely to appear/occur?
- happens when a positive cation polarises a negative ion and pulls its electrons towards ITSELF
- small cation as the positive charge is more concentrated in a smaller area
- larger anion as the outer electrons are less attracted to the nucleus and so can be polarised more easily
- large charge on either ion as this means a stronger ELECTROSTATIC force of attraction and therefore polarisation
what is the name for a single bond?
how does a sigma bond with S orbitals come about?
how does a sigma bond with P orbitals come about?
what is the name for a double bond?
how does a pi bond with P orbitals come about?
what is a dative covalent/coordinate bond?
what is a requirement for this bond to occur?
what symbol would you use to represent this bond? what does the symbol show?
- sigma bond
- orbitals overlap and there is a sharing of electrons
- orbitals overlap head to head and there is a sharing of electrons
- pi bond
- orbitals overlap sideways
- both pairs of electrons are donated from 1 atom to another
- lone pairs
- arrow, shows where the electrons ARE GOING FROM AND TO
what structure comes about from metallic bonding?
how would you describe the structure?
what is holding the lattice in place aka holding the cations and delocalised electrons?
what are 3 factors that dictate the strength of a metallic bond?
explain why they are malleable and ductile
- giant metallic structure
- regular rows of positive metal ions and a sea of delocalised electrons
- strong electrostatic forces of attraction
- the higher the charge density, the stronger the metallic bond
- the number of delocalised electrons depending on the group number
- size of the ion
- regular rows of positive ions can slide over each other without breaking the metallic bonds
reduce the number of lone pairs you have by…
- 2.5
what is electronegativity?
what element is the most electronegative?
electronegativity increases as you go along the period why?
decrease as you go down the group?
electronegativity excludes what group?
what does “polar covalent” or “polar covalent bond” mean
if the difference in electronegativity in ionic is dramatic what’s it like in covalent?
why does co2 have polar bonds but is not a polar molecule?
hydrogen chloride has one polar bond and so has an overall ______ and a dipole ______
note: refer to water as non linear
- the power of an atom in pulling a pair of electrons in a covalent bond towards itself
- fluorine
- number of protons increase
- shielding increases
- noble gases
- electrons being pulled closer to one atom than the other. electrons are unevenly shared/distributed TOWARDS THE MORE ELECTRONEGATIVE ATOM
- similar
- polar bonds in opposite directions and so cancel each other out
- overall polarity, dipole moment
what are the 3 types of intermolecular forces?
- vdw, permanent dipole, hydrogen bonding
