The document discusses covalent bonding. Covalent bonding occurs when atoms share electron pairs to achieve stable electron configurations, rather than gaining or losing electrons like in ionic bonding. Chlorine (Cl2) forms a single covalent bond by each chlorine atom sharing one electron pair. Oxygen (O2) forms a double covalent bond, with each atom sharing two electron pairs to fill its octet. Covalent bonding allows for a diverse array of compounds from small molecules like water to large complex molecules like proteins.
This slides demonstrate on the formation of positive and negative ions, followed by formation of ionic bonding and covalent bonding. Chemical bonding have various types of bonding. In the presentation, we're sharing only ionic and covalent bonding only.
This slides demonstrate on the formation of positive and negative ions, followed by formation of ionic bonding and covalent bonding. Chemical bonding have various types of bonding. In the presentation, we're sharing only ionic and covalent bonding only.
The electrons which are involved in bond formatio.pdfrakeshankur
The electrons which are involved in bond formation between atoms are found in the
outermost shell (sometimes in the next to the outer-most shell) of the neutral atom; these are
called VALENCE ELECTRONS. The atoms of elements which have only one or two electrons
in their outermost shells (active shells) may lose electrons when they combine with atoms of
other elements. An atom which has lost one or more valence electrons possesses a positive
charge, and is called a POSITIVE ION. The sodium atom loses its one valence electron and
acquires a +1 charge when it enters into chemical combination with an atom of an element such
as chlorine. The magnesium atom may lose its two valence electrons and assume a +2 charge.
Na Na+ + e- The Na symbol to the left of the arrow represents a stable sodium atom while the
Na+ symbol to the right of the arrow represents an unstable sodium ion which has had a single
electron removed. Mg Mg++ + 2e- The Mg symbol to the left of the arrow represents a stable
magnesium atom while the Mg++ symbol to the right of the arrow represents an unstable
magnesium ion which has had two electrons removed. The smaller the number of valence
electrons in the atom, the greater the tendency of the element to lose electrons and thus form
positive ions during chemical combination with atoms of other elements. The energy required to
remove an electron from a neutral atom to form a positive ion is called the IONIZATION
POTENTIAL of the atom. Some metals have small ionization potentials and readily form
positive ions. The nonmetals, which have more electrons in their outer shells than the metals,
have large ionization potentials and show little tendency toward the formation of positive ions.
Atoms which lack one or two electrons of having an outermost shell of eight electrons readily
gain sufficient electrons from certain other atoms, such as sodium and magnesium, to make a full
compliment of eight electrons in the outside shell. Neutral atoms become NEGATIVE IONS by
gaining electrons. The nonmetals, such as Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I),
Oxygen (O), Nitrogen (N) and Sulfur (S), readily form negative ions. Cl + e- Cl- Chlorine,
when in its stable form, possesses seven valence electrons and therefore has the ability to gain
one electron (as represented to the left of the arrow) giving it a negative charge of one when in
its unstable ionic form (as represented to the right of the arrow above). S + 2e- S-2 Sulfur, when
in its stable form, possesses six valence electrons and therefore has the ability to gain two
electrons giving it a negative charge of two when in its unstable ionic form. The attraction of a
neutral atom for electrons is known as its ELECTRON AFFINITY. The nonmetals have high
electron affinities and the metals have very low electron affinities. Thus, mainly the nonmetals
tend to form negative ions during chemical combination. When a positive ion and a negative ion
are brought close together, strong electr.
chemical bonding and molecular structure class 11sarunkumar31
hybridisation, bonding and antiboding, dipole moment, VSPER theory, Molecular orbital diagram, Phosphorous pentachloride, ionic bond, bond order, bond enthalpy, bond dissociation, sp and sp2hybridisation, hydrogen bonding,electron pair,lone pair repulsion, resonance structure of ozone, how to find electron pair and lone pair, sp3 hybridization of methane.
CH 4 CHEMICAL BONDING AND MOLECULAR STRUCTURE.pdfLUXMIKANTGIRI
English chapter we will discuss about bonding how the molecules and the ions are in texting as a molecule make the structure there energy their transmission and other
15. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule).
16. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair.
17. In covalent bonding, atoms still want to achieve a noble gas configuration(the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair. The shared electron pair is called a bonding pair
64. There are an estimated 10 40 possible compounds containing up to 50 atoms The known chemical world, including natural and synthetic compounds, is far far far below 1% of that.
65. As of 2007, there are about 31,000,000 known compounds; About 12.5 million of those are commercially available. Thousands of new compounds are discovered or synthesized every week !