Tissues are grouped together to form varius what?
1 answer:
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Answer:
1) 1.202 L
, 2) 1.291 dg
, 3) 204.877 and 4) 1.04x
Explanation:
You need to review about conversion factors and how to use them in the correct order. You can cancel the units and get the ones that you need if you use the appropriate conversion factors, remember is a number that you can use to multiply or divide.
For your exercise:
1) The conversion factor is: 1 L = 1000 mL
You will need to divide by 1000 mL to obtain liters L
1202.57120 mL x = 1.202 L
2) The conversion factor is: 1 g = 10 dg
0.1290743 g x = 1.291 dg
For the next exercises, you need to follow some rules:
1. All numbers that are different from Zero (non-zero digits) are significant figures.
2.The Zeros between non-zeros digits (Imbedded zeros) always are significant, 2007.
3. If you want to be specific and want some zeros to be significant you need to add a decimal point. For example 500. or 500.0
4. Leading zeros (to the left) are not significant.
5. Trailing zeros (zeros to the right) in a whole number without decimal point are not significant.
3) 843.062 - 638.1848 = 204.8772
Now if we round to 6 significant figures we get 204.877
4)123.0 x 8.43 = 1036.89
Now we round to 3 significant figures because 8.43 has the least significant figures.
1.04x
Answer:
<h3>1)</h3>Structure One:
- N: -2
- C: 0
- O: +1
Structure Two:
- N: 0
- C: 0
- O: -1
Structure Three:
- N: -1
- C: 0
- O: 0.
Structure Number Two would likely be the most stable structure.
<h3>2)</h3>- All five C atoms: 0
- All six H atoms to C: 0
- N atom: +1.
The N atom is the one that is "likely" to be attracted to an anion. See explanation.
Explanation:
When calculating the formal charge for an atom, the assumption is that electrons in a chemical bond are shared equally between the two bonding atoms. The formula for the formal charge of an atom can be written as:
.
For example, for the N atom in structure one of the first question,
- N is in IUPAC group 15. There are 15 - 10 = 5 valence electrons on N.
- This N atom is connected to only 1 chemical bond.
- There are three pairs, or 6 electrons that aren't in a chemical bond.
The formal charge of this N atom will be .
Apply this rule to the other atoms. Note that a double bond counts as two bonds while a triple bond counts as three.
<h3>1)</h3>Structure One:
- N: -2
- C: 0
- O: +1
Structure Two:
- N: 0
- C: 0
- O: -1
Structure Three:
- N: -1
- C: 0
- O: 0.
In general, the formal charge on all atoms in a molecule or an ion shall be as close to zero as possible. That rules out Structure number one.
Additionally, if there is a negative charge on one of the atoms, that atom shall preferably be the most electronegative one in the entire molecule. O is more electronegative than N. Structure two will likely be favored over structure three.
<h3>2)</h3>Similarly,
- All five C atoms: 0
- All six H atoms to C: 0
- N atom: +1.
Assuming that electrons in a chemical bond are shared equally (which is likely not the case,) the nitrogen atom in this molecule will carry a positive charge. By that assumption, it would attract an anion.
Note that in reality this assumption seldom holds. In this ion, the N-H bond is highly polarized such that the partial positive charge is mostly located on the H atom bonded to the N atom. This example shows how the formal charge assumption might give misleading information. However, for the sake of this particular problem, the N atom is the one that is "likely" to be attracted to an anion.