For the s block metals (grous 1 and 2) a simple explanation is that the elements with the highest number of valence electrons have the stronger bonds.
For the transition metals the situation is more complicated as well as the s electrons, d electrons are involved and these form more localised bonds of a covalent nature.
For the other metals the description of the bonding is also complex- just to take one examle, gallium is unusual as it has short distances between pairs of Ga atoms - indicating a degree of covaency- hence the low melting point- in the melt it behaves as typicl metal and so has a high b. pt.
Non metals usually form covalent bonds with other non metals and ionic bonds with reactive metals.
The answer expected here is non-metal, and examples are carbon, chlorine, sulfur phosphorus. Metals have metallic bonds. However there are compounds where atoms of a metallic element form covalent bonds to other atoms of the same element.
Metallic bond, metallic positive grains surrounded by the electron cloud
Zinc, as with all metals, reacts to form ionic bonds with other elements.
Oxygen can form both metallic and covalent bonds, depending on the specific elements it interacts with and the conditions under which the bonding occurs. Covalent Bonds: In its most common form, oxygen forms covalent bonds with other nonmetals. For example, in a molecule like oxygen gas (O2), two oxygen atoms share electrons through covalent bonds. This sharing of electrons creates a stable molecule. Metallic Bonds: Oxygen can also form metallic bonds with certain metals. Metallic bonding occurs when electrons are free to move throughout a metal lattice, creating a "sea" of electrons that are shared by all the atoms in the metal. Oxygen can be a part of such a metallic lattice in compounds known as metal oxides. For example, in rust (iron oxide), oxygen forms a metallic bond with iron atoms. So, to sum it up, oxygen primarily forms covalent bonds with nonmetals and metallic bonds with some metals in the context of metal oxides.
because some metals have a stronger attraction toward each other, its just a natural occurence. there is no scientific explanation. generally the shinier the metal is, the more likely it will be to attract to another element.
Metal atoms are bonded each other with metallic bonds. A special feature in metallic bonds is the existence of 'pool of electrons'. It is responsible for the conductivity of electricity and heat in metals.
No. Titanium is an element, not a compound. Like other metals, it is held together by metallic bonds, which are different from covalent and ionic bonds.
All metals form metallic bonds with other metal atoms.
Typically metals form ionic bonds with non- metals. There are exceptions when the metal ion is small and highly charged when the bond may have more covalent character, (Fajans rules) Metals also form covalent bonds with carbon in organometals such as grignard reagents. Transition metals form covalent bonds with many species, e.g. carbon monoxide in the carbonyls. In alloys which are mixtures of metallic elements the bonding is the metallic bond.
No. The noble gasses will not form bonds with most elements and never bond with metals. Metals form metallic bonds with one another, but this is considered a mixture rather than a new chemical compound.
Covalent and ionic. (The other major type of bond, metallic, does not occur in compounds but only in elemental metals and in mixtures of metals.)
Metallic bond is an electrostatic interaction between the metal ions and a sea of free electrons. Mercury is the only liquid metal, whereas all other metals are solids.
Non metals usually form covalent bonds with other non metals and ionic bonds with reactive metals.
The answer expected here is non-metal, and examples are carbon, chlorine, sulfur phosphorus. Metals have metallic bonds. However there are compounds where atoms of a metallic element form covalent bonds to other atoms of the same element.
Metallic bond, metallic positive grains surrounded by the electron cloud
Zinc, as with all metals, reacts to form ionic bonds with other elements.