C2 - atoms, elements & compounds (Ionic, covalent, metallic, giant covalent) Flashcards
what are 2 types of mobile charge carriers
-ions
-electrons
what must all ions have
a complete electronic configuration
define lattice
regular arrangement of alternating positive and negative ions.
define an ionic bond
-transfer of electrons between positive metal ions and negative non metal ions
-forms basic compounds
what is the structure in an ionic bond
lattice structure in regular arrangement of alternating ( + ) & ( - ) ions
What holds an ionic bond together
electrostatic forces of attraction between positive metal ions and negative non metal ions
properties of ionic bonds
-Low volatility
-high solubility
-high melting and boiling point
-conducts when molten or aqueous
Metals lose electrons to? (ionic)
form positive ions
non metals gain electrons to?(ionic)
form negative ions
which shell is the electron lost from or added to
valance shell
if 2 diff atoms of same element have the same electronic configuration as ions, are they the same?
no because the proton numbers are diff.
explain the melting and boiling point of an ionic bond
high because the strong electrostatic forces of attraction between positive metal ions and negative non metal ions require a lot of energy to overcome
explain when and how electricity is conducted in an ionic bond
only when aqueous or molten because that is when the ions are mobile and can carry charge through the structure
Which diagram is used in ionic and simple covalent bonding
dot and cross
when explaining the dot and cross of an ionic bond what are the 4 things needed to say
-total number of electrons in each element and in each shell
-how much electron needed to fill the valance shell of the element
-therefore, how many atoms are needed
-gained = positive metal ions
lost = negative non metal ions
when writing the dot and cross of ions on the electrons transferred, what goes first- number or charge
number
eg, 2+
when finding the number of atoms needed in an ionic dot and cross, what must you try to find
LCM of the numbers of electrons needed by the non metal and metal
define / describe metallic bond
a lattice of positive metal ions in a ‘sea’ of delocalised electrons held by electrostatic forces of attraction
what is the structure in an metallic bond
lattice
what holds metallic bonds together
electrostatic forces of attraction between positive metal ions and a ‘sea’ of delocalised electrons
are metallic bonds good conductors of heat and electricity
yes. they have delocalised electrons which are mobile and can carry charge or heat energy through the structure.
explain the melting and boiling point of metallic bonds
high, strong electrostatic forces of attraction between positive metal ions and a ‘sea’ of delicalised electrons require a lot of energy to overcome
explain the malleability of metallic bonds
they are malleable, metals have a regular structure with layers that can slid off each other
name the 9 properties of metals
-good conductors of heat
-good conductors of electricity
-ductile
-malleable
-some are magnetic (iron, cobalt, nickel)
-high melting and boiling points (usually solids at room temp. except mercury)
define ductile
can be drawn into wires
define malleable
can be bent or hammered into shape
which metals are magnetic
iron, cobalt, nickel
define a covalent bond
shared pair of electrons between non metals
what are the 2 types of covalent bonds
-simple covalent, giant covalent
-forms acidic compounds
what is the structure of simple covalent bonds
small molecules
what holds simple covalent bonds together
-many strong covalent bonds (intramolecular forces of attraction) between atoms
-intermolecular forces of attraction between molecules
which forces are weakened or broken when heating
intermolecular forces of attraction
explain the melting and boiling point of simple covalent bonds
low, the weak intermolecular forces of attraction between molecules require little energy to overcome
can simple covalent structure conduct electricity
no, there are no mobile charge carriers
what is the structure of giant covalent
macromolecule
what holds giant covalent bonds together
-MANY strong covalent bonds (intramolecular forces of attraction) in -between atoms
-no intermolecular forces of attraction
explain the melting and boiling point of giant covalent bonds
high, there are MANY strong covalent bonds in between atom which require a lot of energy to overcome
name 2 giant covalent structures
diamond, graphite
list the physically properties of diamond
-hard (cant be scratched easily)
-high melting and boiling points
-no electricity conduction
-shiny
list all the important notes on diamond
-hard (cant be scratched easily)
-high melting and boiling points
-no electricity conduction
-shiny
-used as a cutting tool
-has MANY strong covalent bonds
-each carbon atom is bonded to 4 other carbon atoms
list the physically properties of graphite
-soft and slippery
-high melting and boiling point
-can conduct electricity
-dull
list all the important notes on graphite
-soft and slippery
-high melting and boiling point
-can conduct electricity
-dull
-used as a lubricant
-has MANY strong covalent bonds
-each carbon atom is bonded to 4 other carbon atoms (so 1 delocalised electron)
-has layers
can giant covalent structures conduct electricity
only graphite because graphite has delicalised electrons which are moblile and can carry charge through the structure
what is the solubility of covalent compounds
low, they do not dissolve in water easily
what is the volatility of covalent compounds
high, they turn into gas easily.
what do you need to think about when drawing dot and cross of simple covalent
-number of electrons in valance shell of each element
-number of electrons needed
why does bromine have a low boiling point
-bromine is a covalent bond
-bromine is non-metal
-it requires little energy to overcome intermolecular forces of attraction btw molecules.
when explaining a propriety of an molecule, what must you say at first about it
the type of bond it is
