Hi! Good morning! I was suppose to turn in this test yesterday. Can You please help me with these last two essay questions. The first one I got the answer, just please tell me if it is correct and the second I don't know the answer. Please help ASAP! Thank you!
Moving from the element with atomic number 10 to atomic number 11 on the periodic table, there is a change in reactivity. In three to five sentences, identify the direction of the change, and give two reasons for the change.(4 points)
My answer: The change in atomic number from 10 to 11 makes a change from a noble gas to a highly reactive group in 1 element. The result of this leads to reactivity increases. The atomic number of an element tells us the group in which the element would go on on the periodic table. An atomic number of 10 shows a outermost filled shell which is a trait of many noble gases.So as we move to an atomic number of 10 to 11 the result would lead to positive reactivity increase.
The periodic table is arranged by various patterns. Is there a pattern with regard to ionic charge? In three to five sentences, explain your reasoning and provide specific examples.
As you complete your response keep in mind that not all elements, commonly the Carbon elements within Group 14, form ionic bonds.
(4 points)
Your answer to the first essay question is partially correct. Moving from the element with atomic number 10 (neon) to atomic number 11 (sodium), there is indeed a change in reactivity. However, it is incorrect to say that it changes from a noble gas to a highly reactive group in one element. The change is actually from a noble gas (with a full outer electron shell) to an alkali metal (with one valence electron). This change leads to an increase in reactivity. A valence electron is more easily lost than the electrons in a filled outer shell, so sodium is more likely to participate in chemical reactions.
For the second essay question, regarding whether there is a pattern with regard to ionic charge in the periodic table, there is indeed a pattern. Ionic charge generally increases as you move from left to right across a period on the periodic table. This is because the number of valence electrons increases from left to right, making it easier for elements to either gain or lose electrons and form ions. For example, in Group 1, the alkali metals such as sodium (Na) have a +1 charge when they lose their sole valence electron. In Group 17, the halogens such as chlorine (Cl) have a -1 charge when they gain an electron to achieve a full valence shell. However, it is important to note that not all elements form ionic bonds, especially the carbon elements in Group 14, which are more likely to form covalent bonds.