chemical bonding and structure

ionic compounds
1, what holds the cations (+) and anions (-) together?
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ionic compounds
1, what holds the cations (+) and anions (-) together?
giant ionic lattice structures
1, strong electrostatic forces of attraction, ie. ionic bonds
why do they have high melting/boiling points?
electrostatic force of attraction between the ions are very strong, therefore, a lot of heat is required to weaken the bond and change the state of the ionic compound from solid to liquid.
does GILS exist in solids, liquids, gases?
only solids
what does the presence of water molecules do to do the structure of solid?
The positively-charged side of the H2O molecules are attracted to the negatively-charged chloride ions and the negatively-charged side of the water molecules are attracted to the positively-charged sodium ions. ... Water molecules pull the sodium and chloride ions apart, breaking the ionic bond that held them together.
how does presence of water molecules make liquids good electrical conductors?
1, absence of what force?
2, what does this do to their movement ?
no strong electrostatic force- -
ions are now not in fixed position
free to move to conduct electricity
why are most ionic compounds soluble in water?
1, what are water molecules attracted to
2, what force between the (+) and (-) charged ions is weakened because of this
3, what structure are ions pulled away from ? what happens to the compound to form an aqueous solution
1, ions
2, electrostatic force
3, GILS, dissolve
1, why is melting pt of magnesium oxide (doubly charged) higher than sodium chloride (singly charged)?
1, charge of an ion in ionic compounds affect the strength of ionic bonds
2, more charged, stronger ionic bonds
simple molecular structures:
there are 2 types of attractions between 2 things which take place at 2 diff places
1, (hint: covalent bonding), strength?, between who and who? where?
2, (hint:among pairs of molecules), strength? where?
1, strong forces of attraction between both non-metal ions
2, weak forces among them.
during melting/boiling:
1, only one type of attraction force is overcome, which one?
2, why can't the other type of attraction force be overcome
1, only attraction between pairs of molecules overcome
2, heat energy not enuf to break covalent bond between atoms
r/s between electrons shared and strength of bond between pairs of molecules ?
...
why poor electrical conductivity for simple molecular structuresneutral particles, no charges, because have full valence shell upon sharing electrons, cannot act as charge-carriers to conduct electricitywhy are covalent molecules electrically neutral meaning their no. of protons= no. of electrons ?non-metals share electrons with each other, not GIVE. so their no. of electrons is not affected. not isotopescan covalent bonding happen in metals? or only non-metalscan only happen between 2 non-metals, ranging from 1-3 covalent bondswhy do metals (metallic structure) have a sea of delocalised electrons? 1, related to their loss of electrons in metals - WHY do metals lose electrons? - based on their group in periodic tableall elements from group I to III have positive charges, meaning that they have given up some of their electrons in order to get a full valence shell. the electrons that they have given up becomes delocalised electrons, forming a sea of free-moving electronshow does the metallic structure (crystal) stay in shape? 1, related to the forces of attractionthe strong electrostatic forces of attraction between the (-) charged delocalised electrons and the metal ion (cation)-ion with (+) charges after losing electronswhy is metallic structure malleable?what happens to ionic compound when electricity passes through them? 1, pertaining to their structure/ element 2, which ions go to the positive terminal of the battery, vice versa?1, they decompose into their elements 2, positive ions go to (-) terminal of battery, negative ions go to (+) terminal of battery