I'm not sure, but once my oven element burned out. I had to replace it, but once I did I made some awesome meatloaf.
The oxygen group of elements form 2- ions. Oxygen, Sulfur, Selenium, Tellurium, Polonium.
Yes.
The ionic charges of group 1 and 2 metals are +1 and +2 respectively. Group 15 & 16 the simple mono-atomic ions are -3 and -2. Group 17 ions are -1. This can be explained by the following elemnts in groups 1 and 2 lose 1 or 2 electrons respectively to achieve a noble gas configuration whereas groups 15, 16 and 17 gain electrons (3,2 1 respectively)
elements of group 6 - colloum 10 gain 2 valence electrons when they form ionic bonds
The elements of group VI A require two electrons to complete the octet so they mostly form -2 ions as O-2, S-2
Potassium will form ionic compound with group 17 elements (fluorine, chlorine, bromine, iodine) and group 16 elements (oxygen, sulphur, selenium).
Group 1 or group 2 elements with group 16 or group 17 elements. In general, if the electronegativity difference between the two atoms is more than 1.7 in Pauling's scale, then the two atoms form ionic bond.
The group 2 elements form ions with a 2+ charge. For example, Mg2+ and Ca2+. The group 16 elements form ions with a 2- charge. For example, O2- and S2-.
The ionic charges of group 1 and 2 metals are +1 and +2 respectively. Group 15 & 16 the simple mono-atomic ions are -3 and -2. Group 17 ions are -1. This can be explained by the following elemnts in groups 1 and 2 lose 1 or 2 electrons respectively to achieve a noble gas configuration whereas groups 15, 16 and 17 gain electrons (3,2 1 respectively)
For the most part, Group 16 forms -2 ions, therefore they most readily bond with Group 2, which primarily form +2 ions.
elements of group 6 - colloum 10 gain 2 valence electrons when they form ionic bonds
The elements of group VI A require two electrons to complete the octet so they mostly form -2 ions as O-2, S-2
Group 16 or the chalcogens.
Potassium will form ionic compound with group 17 elements (fluorine, chlorine, bromine, iodine) and group 16 elements (oxygen, sulphur, selenium).
Group 1 or group 2 elements with group 16 or group 17 elements. In general, if the electronegativity difference between the two atoms is more than 1.7 in Pauling's scale, then the two atoms form ionic bond.
group 16
An element should release two of its outermost electrons to obtain +2 ion. The elements in group 2A are the most likely elements to have this configuration. These are known as Alkali Earth Metals.The elements in the 2nd group have 2 valence electrons. Elements give away their valence electrons to get stable electron configuration. The elements in the 2nd group such as beryllium, magnesium, calcium, strontium, barium likely to have positive ion with charge of 2.Group II elements (the alkaline earth metals). This is because this particular group of elements have two extra electrons in their electronic configurations. They need to lose these two electrons to attain the stable noble gas configuration. So they will have a tendency to lose them to other atoms or group of atoms, in the process incurring a double positive charge (since there will now be two less electrons than protons). So Be, Mg and Ca will all form positive ions (cations) with a charge of +2. They are represented by Be2+, Mg2+ and Ca2+ respectively. But, other elements like copper and barium will also form cations of charge +2.
chalcogens
Group 1 and 2 elements have 1 and 2 valence electrons respectively. Removal of these electrons will result in stable noble gas electronic configuration. Group 17 and 16 elements have 7 and 6 valence electrons respectively. Addition of 1 or 2 electrons to group 17 and 16 respectively will give them stable noble gas configuration. Hence these two groups are highly reactive and their elements will combine to form large number of compounds.