Answer: Some are solid, some are gaseous, a few are liquid. Some are metallic: they have a peculiar lustre; some are coloured (like sulfur) or colourless. Some have a low density; some have a high density. Some are malleable and ductile; some are brittle. Some conduct electricity and heat well; some don’t.
Many metals tend to have structural uses. Nonmetallic elements less so.
Metals tend to have crystal forms featuring close-packed centro-symmetrical structures. Nonmetallic elements tend to have crystal structures featuring more open and directionally packed structures.
Some are especially toxic; some are essential to life; some are both depending on exposure level.
Most are stable; some are less so.
Some elements are highly reactive; some are almost inert (helium, neon, and argon may be completely inert in ambient conditions).
Many metals have basic oxides; quite a few oxides of nonmetallic elements form acids when they are dissolved in water. Some elements can go both ways.
There are many generalisations you can make about metallic and nonmetallic elements, and quite a few exceptions at the margins.
Explanation:
Answer:
closer to F because fluorine has a higher electronegativity than carbon
Explanation:
Electronegativity refers to the ability of an atom in a bonding situation to draw the shared electrons of the bond closer to itself.
Electronegativity increases across the period and decreases down the group. A highly electronegative atom draws the shared electron pair of a bond towards itself.
When two atoms are bonded together, the electron pair is always drawn closer to the atom that has a higher electronegativity.
Hence, the electron pair in a C-F bond could be considered closer to F because fluorine has a higher electronegativity than carbon.
Written Answer: Covalent bonds hold atoms together in molecules and polyatomic ions where as intermolecular forces hold molecules together in a liquid or solid. Intermolecular forces are generally much weaker than covalent bonds.
Explanation/Evidence: "In contrast to intramolecular forces, such as the <u>covalent bonds that hold atoms together in molecules and polyatomic ions</u>, <u>intermolecular forces hold molecules together in a liquid or solid.</u> <u>Intermolecular forces are generally much weaker than covalent bonds."</u>
Then, 
The reaction is as bellows:
1 mole
reacts with 1 mole 
Therefore,
Then, unreacted 
Volume of the solution = 
Now, molar concentration of 
completely dissociates in solution.
Therefore,![[NaOH]=[[OH-]=7.46×10^-4 moles/L](https://tex.z-dn.net/?f=%5BNaOH%5D%3D%5B%5BOH-%5D%3D7.46%C3%9710%5E-4%20moles%2FL)
![pOH= -log[OH-]= -log(7.46×10^-4)= 3.12](https://tex.z-dn.net/?f=pOH%3D%20-log%5BOH-%5D%3D%20-log%287.46%C3%9710%5E-4%29%3D%203.12)
Again,
or,
<h3> </h3><h3>
If sodium hydroxide were added to a solution of strong acid, what would happen to the pH of the solution?</h3>
Depending on how much is added, yes. The solution has a pH of 7 if the amount of additional is exactly equal to the amount of acid.
Since is an excess reagent, the solution will become basic if more equivalents of base are added than equivalents of acid, and the pH of the solution will rise above 7.
The solution will be acidic, with a pH lower than 7, if the number of equivalents of acid exceeds that of the that has been added.
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C. Neutrons combined with protons
