1. There has to be 8 valence electrons in order to fulfill the octet rule, this makes an atom/molecule stable. 2. Atoms with < 4 Valence Electrons (VE's) will give up their outer electrons. Atoms with > 4 VE's will collect electrons to make a full set of 8. 3. The charge is considered by whether there's more protons, positively charged, or electrons, negatively charged. Confusion: There was no confusion, every single part of it was easy for me. Question: Is it possible for us to discover any more elements? ADC
I found it was interesting how the noble gases are like the stars on the periodic table, because all the other electrons want to be like the noble gases because they have 8 valence electrons and they don'e have to lose any. Metals are easy because they will always lose electrons. I wonder if the elements will either have twelve electrons or four because twelve minus four is 8 and 4 plus 4 is 8. This guy did a good job explaining i took a lot of notes. Alex it is possible for us to discover more electrons.
The octet rule says that in order to have an outer shell of 8, atoms will be lost or gained. The full outer shell is stable. On the periodic table, each row (1, 2, 3, 4, 5, 6, 7, 8) is the number of outer shell electrons. The group number tells how many electrons there is on the outer shell. Elements with 4+ valence electron FILL. Elements with 4- valence electrons FALL back to the core octet. I wonder how many elements we haven't discovered yet, if any. JJP
I observed that all noble gases on the periodic table are stable. Another words noble gases have all the valence electrons that they want, which is 8. I learned that if an atom has less than four electrons in its outer shell, then it will lose those electrons so a new energy level will be made, (which has eight electrons). If an atom has more than 4 electrons, it will gain electrons so that it could have an octet. I am confused on all of the numbers he was labeling the electrons with, like 1s2Ps2...what does that mean? My question is if an atom just had 4 valence electrons would it lose or gain electrons. The man said if an atom had more or less of 4 electrons, but what if an atom had just 4 electrons? MJS
this like the other video was very easy to under stand. we learned the octet rule which i think he did better than mr.Ross. i wonder if there is any way to make a bigger element than this bmm
This video was kind of hard to understand because the man was writing things down really small, so it was hard to read what he was writing, and when I could see what he was writing, it was something like 1s2ps2 or L3. He never explained what any of that meant, so it got a little confusing. He did a good job of simplifying things, so i got a better understanding of the octet rule, and I thought it was really interesting that they can lose an entire outer shell! That means that they can be different sizes, which I also did not know. JMJ
I found it interesting how he showed the different energy levels on magnesium. I think that this video was to simple, he used simple word's compared to the first video. his voice sounded weird. how come in most videos do they erase the Transition Elements. E.D.B
over all pretty boring I was really hard to under stand what he was saying and it was also really hard to under stand what math was going on in the video to
The noble gases are the only elements with with a full set of electrons. All the others try to be like that. To get a full set of electrons, they will either gain or loose them. but if an element wants a full set of electrons, then how could they possibly stand to loose any? if it has <4 valence electrons, then it will give up its outer electrons. If it has >4valence electrons, then it will try to gain more by sharing with others. I was surprised to find out that the answered to his question was that magnesium would loose electrons rather than gain them but that was before I found out why. Although it was odd to me, I learned how you know if an element gains or looses electrons. L.G.D.
1. There has to be 8 valence electrons in order to fulfill the octet rule, this makes an atom/molecule stable.
ReplyDelete2. Atoms with < 4 Valence Electrons (VE's) will give up their outer electrons. Atoms with > 4 VE's will collect electrons to make a full set of 8.
3. The charge is considered by whether there's more protons, positively charged, or electrons, negatively charged.
Confusion: There was no confusion, every single part of it was easy for me.
Question: Is it possible for us to discover any more elements?
ADC
I found it was interesting how the noble gases are like the stars on the periodic table, because all the other electrons want to be like the noble gases because they have 8 valence electrons and they don'e have to lose any. Metals are easy because they will always lose electrons. I wonder if the elements will either have twelve electrons or four because twelve minus four is 8 and 4 plus 4 is 8. This guy did a good job explaining i took a lot of notes. Alex it is possible for us to discover more electrons.
ReplyDeleteThe octet rule says that in order to have an outer shell of 8, atoms will be lost or gained. The full outer shell is stable.
DeleteOn the periodic table, each row (1, 2, 3, 4, 5, 6, 7, 8) is the number of outer shell electrons. The group number tells how many electrons there is on the outer shell.
Elements with 4+ valence electron FILL. Elements with 4- valence electrons FALL back to the core octet.
I wonder how many elements we haven't discovered yet, if any.
JJP
I observed that all noble gases on the periodic table are stable. Another words noble gases have all the valence electrons that they want, which is 8. I learned that if an atom has less than four electrons in its outer shell, then it will lose those electrons so a new energy level will be made, (which has eight electrons). If an atom has more than 4 electrons, it will gain electrons so that it could have an octet. I am confused on all of the numbers he was labeling the electrons with, like 1s2Ps2...what does that mean? My question is if an atom just had 4 valence electrons would it lose or gain electrons. The man said if an atom had more or less of 4 electrons, but what if an atom had just 4 electrons?
ReplyDeleteMJS
this like the other video was very easy to under stand.
ReplyDeletewe learned the octet rule which i think he did better than mr.Ross.
i wonder if there is any way to make a bigger element than this
bmm
This video was kind of hard to understand because the man was writing things down really small, so it was hard to read what he was writing, and when I could see what he was writing, it was something like 1s2ps2 or L3. He never explained what any of that meant, so it got a little confusing. He did a good job of simplifying things, so i got a better understanding of the octet rule, and I thought it was really interesting that they can lose an entire outer shell! That means that they can be different sizes, which I also did not know. JMJ
ReplyDeleteI found it interesting how he showed the different energy levels on magnesium.
ReplyDeleteI think that this video was to simple, he used simple word's compared to the first video. his voice sounded weird.
how come in most videos do they erase the Transition Elements. E.D.B
over all pretty boring
ReplyDeleteI was really hard to under stand what he was saying and it was also really hard to under stand what math was going on in the video to
The noble gases are the only elements with with a full set of electrons. All the others try to be like that. To get a full set of electrons, they will either gain or loose them. but if an element wants a full set of electrons, then how could they possibly stand to loose any? if it has <4 valence electrons, then it will give up its outer electrons. If it has >4valence electrons, then it will try to gain more by sharing with others. I was surprised to find out that the answered to his question was that magnesium would loose electrons rather than gain them but that was before I found out why. Although it was odd to me, I learned how you know if an element gains or looses electrons.
ReplyDeleteL.G.D.