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anonymous
 one year ago
Determine the electronegativity between the atoms of each molecule.
Identify the bond as either ionic or covalent.
State whether the molecule is polar or non polar.
Identify the structure as having hydrogen bonding, dipoledipole moments or London dispersion forces (LDF).
anonymous
 one year ago
Determine the electronegativity between the atoms of each molecule. Identify the bond as either ionic or covalent. State whether the molecule is polar or non polar. Identify the structure as having hydrogen bonding, dipoledipole moments or London dispersion forces (LDF).

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0i need these 4 questions for 4 elements: H2O, NH3, CH4, and CO2

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2An ionic bond is formed when one atom accepts or donates one or more of its valence electrons to another atom. A covalent bond is formed when atoms share valence electrons. The atoms do not always share the electrons equally, so a polar covalent bond may be the result.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0so which element has covalent bonds?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0It'll probably help to look at the Lewis structures of these compounds, as well as an electronegativity chart (all of which you can find online).

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2The ones with covalent bonds are the ones that share their electrons

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0i already have all the lewis structures in front of me

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2Yes all are covalent bonds of some sort

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ok, and im really having trouble with the electronegativity, how do i calculate that

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2The electronegativity can be found on the periodic table and you subtract the lower one from the higher one

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0so subtract the atomic number from atomic mass?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2No there is a Number on the back of the periodic table that is the electronegativity of the element you can also search it too

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0and then subtract the electronegativity from the atomic number?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2No you subtract the electronegativities between the two elements

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0im lost.. could you do an example? what two elements are you talking abuit

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2HF H has an electronegativity of 2.20 F has an electronegativity of 3.98 3.982.20=1.78

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ohhh so you always subtract the lesser from the larger? or can you get a negative

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2I don't think there should be a negative i'm pretty sure it is always larger minus smaller

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ok give me a sec to do all 4

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1If \(\sf \Delta EN>1.7\), then the bond must be ionic. For deciding whether the molecule is polar or not, you need to consider the geometry of molecule. If it is symmetrical then its nonpolar otherwise polar. Ih any molecule has a hydrogen atom attached to highly electronegative elements like N, O or F, then there are greater chances of hydrogen bonding.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0H2O: Polar CO2: Nonpolar CH4: Nonpolar NH3: Polar im pretty sure im correct

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1Example, \(\sf NH_3\) EN of N is 3.04 EN of H is 2.2 \(\sf \Delta EN=3.042.2=0.84<1.7\) so the bonds will be covalent

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0they're all covalent

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0oh, i meant 1.24 is what i got after i subtactred them

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1NH3 has a tetrahedral structure with a lone pair, thus it is unsymmetrical and hence has a dipole moment which makes it a polar molecule.

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1For \(\sf H_2O\) there are 2 OH bonds, you need to see if OH bond is ionic or covalent. \(\sf \Delta EN = 3.442.2=?\)

Abhisar
 one year ago
Best ResponseYou've already chosen the best response.1I need to leave now, I'll be back in a hour or so. I'll request @taramgrant0543664 to help you further c:

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2Yes you were correct about which ones are polar and non polar ones

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ok, and i was correct about them all being covalent right

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2Yes they are only polar and nonpolar if they are also covalent

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0and i did the calculations and this is what i got H2O: 1.24 CO2: 0.89 CH4: 0.35 NH3: 0.84
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