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irina1246 [14]
3 years ago
15

which of the following experiments follow ethical standards? A.)performing test on animals when the information can be obtained

in other ways. B.) experiments done to people who cannot protect themselves. C.) Releasing contaminated contaminated waste into the water system. D.) Research on animals in which the animal in which the animal experiences no fear or pain.
Chemistry
2 answers:
Ilya [14]3 years ago
5 0

Answer:

D.) Research on animals in which the animal experiences no fear or pain.

Explanation:

It is ethical to perform test on an animal such that the animal experiences no fear or pain.  

It is unethical to perform test on an animal when some other tests can be performed without the animal to get the desired results.  

Polluting the water resource with contamination is an unethical practice.  

People who are vulnerable cannot be subjected to experiments.  

olasank [31]3 years ago
3 0
The answer is D because it sounds like the most ethical answer. The other choices are wrong because the could possibly hurt someone or an animal.
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B

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State general trend for metal properties as you go left to right across a period
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Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties. Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties. These trends exist because of the similar atomic structure of the elements within their respective group families or periods, and because of the periodic nature of the elements.

Electronegativity Trends

Electronegativity can be understood as a chemical property describing an atom's ability to attract and bind with electrons. Because electronegativity is a qualitative property, there is no standardized method for calculating electronegativity. However, the most common scale for quantifying electronegativity is the Pauling scale (Table A2), named after the chemist Linus Pauling. The numbers assigned by the Pauling scale are dimensionless due to the qualitative nature of electronegativity. Electronegativity values for each element can be found on certain periodic tables. An example is provided below.


From left to right across a period of elements, electronegativity increases. If the valence shell of an atom is less than half full, it requires less energy to lose an electron than to gain one. Conversely, if the valence shell is more than half full, it is easier to pull an electron into the valence shell than to donate one.

From top to bottom down a group, electronegativity decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius.

Important exceptions of the above rules include the noble gases, lanthanides, and actinides. The noble gases possess a complete valence shell and do not usually attract electrons. The lanthanides and actinides possess more complicated chemistry that does not generally follow any trends. Therefore, noble gases, lanthanides, and actinides do not have electronegativity values.

As for the transition metals, although they have electronegativity values, there is little variance among them across the period and up and down a group. This is because their metallic properties affect their ability to attract electrons as easily as the other elements.

According to these two general trends, the most electronegative element is fluorine, with 3.98 Pauling units.



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