What is noticeable about all of the ionic charges in Group 1 2 15 16 and 17?
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)
Zero is always the sum of all charges in a formula for a neutral compound, whether ionic or not.
No, only the K+ ion is possible; this is valid for all other alkali metals (group I)
This sum will be zero.
No. The ratio depends on the charges of the ions.
Every positive charge will cancel out a negative charge so the sum of all charges should be zero.
All metals combine to form ionic compounds. Group 1(except hydrogen),2-12, all elements form ionic compounds. then Group 13 (except Boron), Group 14-tin and lead and Group 15 Bismuth only. The above mentioned group elements form ionic compounds.
Lithium oxide is an ionic compound, further, all oxides of the group 1 elements are ionic.
All group 1 metals and group 2 elements excluding beryllium will form ionic compounds with nitrogen.
They have different ionic charges (positive and negative). Not all ions attract each other, only those with opposing charges do.
Astatine is in the group 7A of the periodic table. The members of this group all have an ionic charge of -1, so At (astatine) will have a -1 ionic charge.
It means that all ionic charges have been equalled by an oppositely charged ion.
because the number of net positive charges (cations) and the negative charges (anions) same. so they are over all neutral
Yes, Sodium forms ionic compounds with everything, all the alkaline metals do. It is one of the properties of the group.
All (group one) alkali-metals form ionic bonds in metal-salts like LiMnO4
Ionic compounds are neutral because the positive and negative charges will arrange themselves to cancel each other out. For instance, in the molecule Magnesium Chloride, magnesium will have a 2+ charge and will bond with two chloride ions (each a 1- charge) so that all the charges will cancel out.
The alkali metals are Lthe group 1 elements are Lithium, Li; sodium, Na; Potassium, K Rubidium, Rb;Caesium, Cs and francium, Fr. They form ionic compounds where they are all have single positive charges.
Iron (II) fluoride All transition metals need roman numerals to represent their charges.
Chemical compounds are electrically neutral. Ionic compounds contain charged ions but these charges always balance out.
Anions have negative charges (extra electrons). Most polyatomic ions and nonmetallic ions are anions. Cations have positive charges (lacking electrons). All ionic metals are naturally cations.
They all bond atoms together. They all do it in different ways. Metallic bonds involve ions in a sea of electrons, Ionic bonds are between ions of opposite charges and covalent bonds involve the sharing of electrons
Halons are a class of element, not a type of charge. As for why the halogens have the most stable charges, they don't - at least not all of them.
AlF3 - Ionic compound ( formula compound) - Type I - Binary ionic compound - Ionic charges Al (+3) and F (-1) - EN (electronegativity) Al is 1.61 - EN (electronegativity) F is 3.98 - the difference in electronegativity is 2.37 The fluorine atom (F) is the most electronegative of all the elements, and the francium atom (Fr) is the least electronegative of all the elements.
No, methanol, CH3OH, is basically a methyl group, CH3 with an attached hydroxyl group. All covalently bonded.
It's a Ionic compound. Lithium gives up it 1 valence electron, so Fluoride takes that lost electron. They become opposite charges and attract each other. That is how it all works.
Fluorine's bonds are technically covalent, but it is such a strongly electron withdrawing group that for all intents and purposes its bonds can be considered ionic.
Short answer both ionic and covalent! The bond between the sodium (metal) and phosphate (PO43-) (nonmetal) is ionic. The bonds between the phosphorous (nonmetal) and the oxygen (nonmetal) atoms are all covalent. The trick is to treat a covalent compound (PO43-, CO32-, etc) as grouped together when balancing charges, looking for ionic bonds, etc.
Non metals gain electrons when ionic bonds are formed. These are group 15 where nitrogen down to antimony gain 3 electrons to form e.g. N3- group 16 where all members from oxygen to polonium gain 2 electrons to form e.g. O2- group 17 where all members of the group gain one electron to form e.g Cl-
All ionic compound are not salts but all salts are ionic compounds for example NaOH is an ionic compound but not the salt.
Sodium polyacrylate is a polymer (a long chain molecule) with ionic groups (negative charges with accompanying positively charged sodium ions) all along its length. It is these ionic groups that allow it to absorb a huge amount of water.
An ionic compound with a polyatomic cation and polyatomic anion The atoms in the anion are all from the same group?
Nh4 +so3 2-
the group number
The most common way to determine the ion of an atom on the periodic table is to look at the group it is in. Moving from left to right the elements will usually have the ionic charges of +1,+2,+3,+-4,-3,-2,-1. All elements in each group will have the same ionic charge . The transition metals are not as easy as this but a general method to use is that most transition metals have a charge of… Read More
All the time.
because all 3 Phosphate group are negatively charges. These charges are crowded together, so their mutual repulsion contributes to the instability of Stop molecules
The molecular equation is just a list of all atoms in a molecule - "NH3" is nitrogen + 3 hydrogen, for instance. The ionic equation also lists the charges of ions, and would generally be written [N-3][3H+] or so, depending on conventions. This notation does not necessarily imply ionic bonding - water, which is covalently bonded, has the ionic equation [O-2],[2H+].
All ionic substances are indeed ionic, that is to say that contain positively charged cations and negatively charged anions. All ionic substances crystallize into small crystal when they are in their solid form
It is ionic, All the compounds of Sodium are ionic.
Ionic. All potassium compounds are ionic.
Ionic. All cesium compounds are ionic.
All groups bond with at least one halogen, with the notable exception of the noble gases where some of the group do not. Group 1 elements (the alkali metals) are all +1, and, because the halogens are -1, will bond with them in a one-to-one ratio. Those bonds are ionic bonds. Group 2 elements (the alkali earth metals) will bond with halogens, and because group 2 elements are all +2, they bond in a one-to-two… Read More
none of the elements in the periodic table have a charge unless they gain (- charge) or lose (+ charge) an electron, or they can get delta charges which depends on what they are bonded too, that is what i learned in A2 chem a few monthes ago The above information is absolutely correct... but here is a bit more information specifically for group 1A elements. All elements in group 1A can have a +1… Read More
To my best knowledge there are NO ionic alcohols at all. It has however a polar group at one end: -CH2OH, being relatively small compared to the other side of the (linear) molcule: -C15H31 which is NON-polar.
Roc Royal......if you check with all the music videos, you can see hes the one who is not quite there yet with the rest of the group. He falls behind and it is really noticeable.
No not necesserily. because isotopes are of two types # Ionic # non-ionic Mainly the ionic isotopes are radioactive. Some non-ionic are also radioactive but not all.
Yes. It is an ionic compound. All metal compound is ionic.
No, all ionic compounds are solids.
All axes are straight. - If the Earth's axis were perpendicular to the plane of orbit, there would be no noticeable seasons. All axes are straight. - If the Earth's axis were perpendicular to the plane of orbit, there would be no noticeable seasons. All axes are straight. - If the Earth's axis were perpendicular to the plane of orbit, there would be no noticeable seasons. All axes are straight. - If the Earth's axis… Read More