can anyone help me with 03.06 COVALENT BONDING AND LEWIS STRUCTURES
I don't really understand what to do and i don't understand the topic
If you would mind posting an example question I'd be happy to take a look at it.
Ok
Which type of compound usually has higher melting points: ionic compounds or covalent compounds? What is the reason for this difference in melting points? (3 points) Do ionic compounds conduct electricity as: (3 points) Solids? Liquids? Aqueous solutions (when the ionic compounds are dissolved in water)? Do covalent compounds conduct electricity as: (3 points) Solids? Liquids? Aqueous solutions (when the covalent compounds are dissolved in water)?
ionic compounds have higher melting points b/c ions bond and form a lattice structure, and to melt an ionic compound, the lattice structure must be disrupted which requires more energy than breaking the bonds in an inoic compound ionic compounds do not conduct electricity as solids (ions are not free to move/carry charge) but do conduct electricity as liquids/aqueous solutions covalent compounds typically do not conduct electricity in any form (no free electrons) hope that helped you can read more about these things here: http://www.bbc.co.uk/schools/gcsebitesize/science/add_ocr_21c/chemical_patterns/group1_7rev5.shtml http://www.bbc.co.uk/schools/gcsebitesize/science/add_edexcel/covalent_compounds/compoundsrev1.shtml
THANK YOU SO MUCH!
Could you help me with one more thing
sure
OK so i am learning about intermolecular forces could you explain it a little better than my lesson
intermolecular forces are attractive/repulsive forces between molecules b/c of permanent or induced charge differences some common types: 1. ion-dipole: forces between ions (which are charged due to the excess or absence of electrons) and dipoles (charged due to unequal distribution of charges within the molecule) 2. dipole-dipole: attractive forces between the positive/negative ends of two polar molecules 3. hydrogen bonding: when a hydrogen atom is bonded to an electronegative atom such as N,O,F, causing a charge separation where the hydrogen atom is more positively charged and the electronegative atom is more negatively charged, making the electronegative atom more susceptible to attracting the positive charge from other hydrogen atoms from different molecules (probably easier to see this w/ a picture) 4. London dispersion forces (sometimes called induced dipole): attractive forces between a dipole and a neutral molecule. the dipole causes a temporary charge separation in the neutral molecule which causes the dipole to be attracted to the neutral molecule (again, this is probably easier to demonstrate w/ a picture)
ion-dipole|dw:1513553065308:dw|
dipole dipole |dw:1513553097332:dw|
hydrogen bonding |dw:1513553120409:dw|
thank you
induced-dipole/london|dw:1513553151464:dw|
I really appreciate your help
can you tell me what the electronegativity of ch4 is
http://www.thecatalyst.org/electabl.html general method: find the difference in electronegativity between the elements using a table like the above ^ look up the electronegativity of carbon, the minus the electronegativity of hydrogen to get your answer
need to get going, I think dude and Shadow are familiar with enough chem to help if you still need more
ok thank you
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