bonding and trends Flashcards
types of elements in metallic bonds
between metal ions
type of elements in ionic bonds
between a metal and a non-metal
types of elements in covalent molecular bonds
non-metals
types of elements in covalent network bonds
non-metals
how are metallic bonds held together
an electrostatic attraction between the delocalised electrons and the positive ions
how are ionic bonds held together
an electrostatic attraction between the positive cations and the negative anions
how are covalent molecular bonds held together
an electrostatic attraction between the positive nuclei and the share pair of electrons
how are covalent network bonds held together
an electrostatic attraction between the positive nuclei and the share pair of electrons
what is the melting point of metallic bonding
high melting point due to the strong electrostatic attraction between the positive metal ions and the negative electrons
what is the melting point of ionic bonding
high melting point due to it having a strong electrostatic between the ions that a large amount of energy is required to remove it
what is the melting point of covalent molecular bonding
low melting point due to the electrostatic attraction in between the molecules being weak
what is the melting point of covalent network bonding
high melting point due to the intramolecular forces being strong so
how are metallic bonds formed
the valence electrons are removed from the cation’s and move freely with a 3D arrangement of the cations
how are ionic bonds formed
the electrons are transferred from the metals to the non-metals
how are covalent molecular bonds formed
two or more atoms will share their valence electrons to gain a full outer shell
how are covalent network bonds formed
two or more atoms will share their valence electrons to gain a full outer shell
can metallic bonds conduct
it is conductivity due to the mobility of the delocalised electrons allowing the heat and electricity to move along the piece of metal
can ionic bonds conduct
won’t conduct electricity if it is a solid since the electrons are in fixed positions but it can conduct if it is in a liquid or aqueous solution state since the electrons are free to move
can covalent molecular bonds conduct
no, since conductivity requires a mobile charged particle to carry the charge. but there isn’t any charged particles in covalent molecular bonds since they are all neutral
can covalent network bonds conduct
non-conductive except graphite, this is since all the electrons are used during intermolecular bonding. so there are no mobile electrons which mean it has a neutral charge
why is metallic bonding malleable
the layers of positive ions can slip and slide past each other while keeping the metallic bond intact
why are metallic bonding ductile
the layers of positive ions can slip and slide past each other while keeping the metallic bond intact
why do metallic bonds have a hard property
the strong electrostatic attraction between the cations and the electrons. this makes it hard to separate the particles from one another
what are some examples of metallic bonding
magnesium, sodium, potassium, lithium
why are ionic bonding hard
hard due to the strong electrostatic between ion
why are ionic bonds brittle
due to the orderly arrangement of the ions. this means that if the layers are forced to slide past each other, the like ions are pushed together, increasing repulsive forces and therefore shattering
which state would you find covalent molecular bonds
most likely to be a liquid or gas at room temperature due to their low melting points.
why are covalent molecular bonds soft
little force is required to push the molecules past each other
why are covalent molecular bonds malleable
mainly in large molecules. they can be pushed past each other due to the weak forces between them
why are covalent network bonds hard and brittle
the strongly bonded atoms are hard to disrupt so they are hard and brittle
why are covalent molecules inert
due to the molecules all being neutral, there aren’t any particles that have a charge
what are the five covalent network bonds
diamond, graphite, silcion carbide, silcion dioxide, boron nitride.
what are some examples of ionic bonding
sodium oxide, potassium chloride, alumium hydroxide
what are some examples of covalent molecular bonding
water, nitrogen oxide, carbon dioxide
what types of substances dissolve in ethanol
types of substances that dissolve in ethanol are organic substances. due to ethanol being an organic substance, only organic substances can dissolve in ethanol. ethanol is organic since it contains carbon molecules. ethanol consists of both polar and non-polar bonds which are why it is organic. ethanol attracts non-polar substances.
what are inorganic substances
any substance that doesn’t contain carbon. for example water. these are inorganic since they only have polar covalent bonds.
what is a polar substance
Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms. polar bonds have a slightly positve and negative charge which attracts the polar water
what is a non-polar substance
two atoms share a pair of electrons with each other
