0
Non metals are likely to steal electron. They form anions.
Wiki User
∙ 9y ago
Wiki User
∙ 7y agoThese are the non-metals, as halogens.elements.
Add your answer:
Earn +20 pts
In terms of electrons in the periodic table why are group 1 metals very reactive and group 7 non-metals very reactive too?
Atomic elements typically want to have full electron shells ("valence shells"), instead of shells with uneven numbers. Group 1 metals have only 1 electron in their valence shell, so they quickly react to lose this electron and have an empty shell (but a full shell underneath it). Group 7 elements have 7 valence electrons and react quickly to steal another atom's electron and gain a full shell of 8 electrons. This willingness to lose or steal electrons makes the elements very reactive, but in different ways. Group 1 elements will become positively charged ions, and Group 7 will become negatively charged. (Na+ versus Cl-) Group 6 elements (such as oxygen) are also somewhat reactive and will steal 2 electrons to become even more negatively charged (O 2-)
Do elements in group 8 readily or rarely form ions?
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
What kind of bonds form when atoms steal electrons?
This is an ionic bond.
Which element group have the most positive electron affinities?
The group that has a substantial affinity for electrons is group 17, the halogens. These elements have 7 valence electrons which makes them have the highest affinity for electrons.
Does the number of valence electrons in an atom of an element determines many properties of the element including the ways in which the atom can bond with other atoms?
Yes. The atom only bonds spontaneously if its to become more stable. So depending on the valence electrons, they have different forms of getting that stability. Let's see: Elements from the first and second group have 1 and 2 electrons of valence, respectively, so they tend to give them up. That's why they tend to bond with ionic bonds. They never steal electrons from others. Elements from the 17th group, are missing one electron to have their valence orbitals full, so again, they tend to steal electrons from those of group 1, forming stable ionic bonds. They can also give up some of their electrons, but more commonly they prefer to steal one. Elements like N and C, have their valence orbitals close to 50% filled, so they tend to prefer sharing electrons, that is, covalent bonds. Finally noble gases, have their valence orbitals filled with electrons, so they don't react with anything, and the only bonds they make, are weak Van der Waal bonds between themselves.
What will chlorine do to become more stable?
'Steal' electrons from other elements where possible, or share them if that is more efficient.
What category of elements on the periofic table tends to create negatively charged ions?
The oxygen, nitrogen, and fluorine groups love to steal electrons from other elements, making them negatively charged ions, whereas most metals up to the carbon group like to give away electrons, making them positively charged ions. I hope that's what you were asking.
Why do elements form ion?
Both of the elements will have two different electronegativities. When there is a large difference between the two electronegativities, one element will "steal" one or more electrons from the other element. The energy required for this is ionization energy, and increases as an element takes more electrons from another. My answer: Elements are stabilized when they contain a "complete shell" or the noble gas configuration of electrons, which is usually eight electrons. Elements that have a number of electrons close to that of a noble gas, will lose or gain electrons easily. For example, elements in the column just to the left of the noble gases have one fewer electron than the noble gas next to it, and therefore they tend to gain one electron easily. Elements in the column on the far left of the periodic table have one more electron than the noble gas in each row, and they tend to lose one electron easily. Because the protons contribute the positive charge, and the electrons contribute the negative charge, an ion is formed when an element gains or loses one or more electrons.
In terms of electrons in the periodic table why are group 1 metals very reactive and group 7 non-metals very reactive too?
Atomic elements typically want to have full electron shells ("valence shells"), instead of shells with uneven numbers. Group 1 metals have only 1 electron in their valence shell, so they quickly react to lose this electron and have an empty shell (but a full shell underneath it). Group 7 elements have 7 valence electrons and react quickly to steal another atom's electron and gain a full shell of 8 electrons. This willingness to lose or steal electrons makes the elements very reactive, but in different ways. Group 1 elements will become positively charged ions, and Group 7 will become negatively charged. (Na+ versus Cl-) Group 6 elements (such as oxygen) are also somewhat reactive and will steal 2 electrons to become even more negatively charged (O 2-)
Do elements in group 8 readily or rarely form ions?
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
What causes an element to be reactive?
In the short form: elements are striving to completely fill valence shells of electrons to reach a quantumly stable energy state. They react to take electrons away from elements willing to give up electrons or share outer shell electrons with elements they aren't strong enough to steal from.
Why is it easy for oxygen to react with other elements?
Oxygen is a really strong oxidizing agent, meaning it's really greedy with electrons. It really wants to become stable like the noble gases, who have completely filled electron shells. The only way to get electrons is to oxidize other elements and steal their electrons. That's why oxygen is so reactive.
When P become a ion it becomes P3- not P5 why?
It is easier for this element, due to its electronegativity, to gain three electrons off other elements then to lose 5 of its own. Its like each elemnt has a strength. How strong an element is causes that element to be able to hold on to its own electrons and even steal electrons from other elements. Phosphorous is a relatively strong element. It can hold onto its original valence electrons quite well and won't let any of them go. It also can steal electrons from other elements that are weak enough to let their valence electrons go. Its like a tug of war. Phosphorous is strong so it holds its own side of rope (its own electrons) and can pull the other side of rope if the other element is weak.
Is a group in the periodic table more reactive near the top or the bottom?
Francium and Flourine are the most reactive elements. Francium is at the bottom, Flourine is at the top. The trend isn't as simple as your question. Elements towards the top of the table "want" electrons more. This means they are less likely to give them up and more likely to "steal." In terms of reactivity, this means that the metals at the top are less reactive and the non-metals at the top are more reactive.
What makes Noble gases different than any other element?
Noble gases differ from other elements in that the number of electrons that are attached to the core is exactly right. Most elements have either too much or too few electrons to fill their shells (rings of electrons surrounding the nucleus). Noble gasses therefore do not interact with other elements to shed, share or steal electrons like other elements do. Under normal conditions these gases do not react with any other element, and it is therefore that no one ever isolated a noble gas until 1895.
Why is a triple bond the most difficult to break?
The main reason for this is because, within the triple bond there is a high concentration of electrons. Therefore, electrophillic elements like oxygen will be attracted to the bond. These elements can steal electrons from the bond and form a related compound. Better answers will probably follow, but this is a start at least.
What compounds steal electrons?
DCPIP acts as an electron acceptor of a Hill Reacton. In this way, it "steals" electrons.
