What kind of elements form covalent compounds

Due to the … From courses. From school-for-champions. In ionic bonding, atoms transfer electrons to each other. Ionic bonds require at least one electron donor and one electron acceptor. In contrast, atoms with same electronegativity share electrons in covalent bonds, because neither atom preferentially attracts or repels share electrons. In this … From plex. Are you curently on diet or you just want to control your food's nutritions, ingredients?

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Ionic bonds; hold atoms together within a molecule B. Intermolecular forces;. The foreces of attraction between molecules of I2 are: covalent bonds ionic bonds dipole-dipole attractions london forces hydrogen bonds. You can view more similar questions or ask a new question. Questions chemistry What kinds of elements form covalent bonds? Similar Questions Chemistry-Bonding Classify the following bonds as ionic, covalent, or neither O, atomic number 8; F, atomic number 9; Na, atomic number 11; Cl, atomic number 17; U, atomic number Na with Na science below are about 21 questions from my final study guide.

Would you expect this compound to have ionic bonds, chemistry The strongest intermolecular forces present in a sample of pure I2 are A. Both between and within Science 1.

The main types of chemical Chemistry Sulfur can form a bond with any of the following elements: oxygen, chlorine, bromine, or phosphorus.

Chemistry which of the following elements does not form bonds easily because it has a full outer shell? When an electron, or dot, from one element is paired with an electron, or dot, from another element, this makes a bond, which is represented by a line Fig. The number of bonds that an element can form is determined by the number of electrons in its valence shell Fig.

Similarly, the number of electrons in the valence shell also determines ion formation. The octet rule applies for covalent bonding, with a total of eight electrons the most desirable number of unshared or shared electrons in the outer valence shell. For example, carbon has an atomic number of six, with two electrons in shell 1 and four electrons in shell 2, its valence shell see Fig.

This means that carbon needs four electrons to achieve an octet. Carbon is represented with four unpaired electrons see Fig. If carbon can share four electrons with other atoms, its valence shell will be full. Most elements involved in covalent bonding need eight electrons to have a complete valence shell.

One notable exception is hydrogen H. Hydrogen can be considered to be in Group 1 or Group 17 because it has properties similar to both groups. Hydrogen can participate in both ionic and covalent bonding.

When participating in covalent bonding, hydrogen only needs two electrons to have a full valence shell. As it has only one electron to start with, it can only make one bond. Hydrogen is shown in Fig 2. In the formation of a covalent hydrogen molecule, therefore, each hydrogen atom forms a single bond, producing a molecule with the formula H 2. A single bond is defined as one covalent bond, or two shared electrons, between two atoms.

A molecule can have multiple single bonds. For example, water, H 2 O, has two single bonds, one between each hydrogen atom and the oxygen atom Fig. Figure 2. Sometimes two covalent bonds are formed between two atoms by each atom sharing two electrons, for a total of four shared electrons. For example, in the formation of the oxygen molecule, each atom of oxygen forms two bonds to the other oxygen atom, producing the molecule O 2. Similarly, in carbon dioxide CO 2 , two double bonds are formed between the carbon and each of the two oxygen atoms Fig.

In some cases, three covalent bonds can be formed between two atoms. The most common gas in the atmosphere, nitrogen, is made of two nitrogen atoms bonded by a triple bond.

Each nitrogen atom is able to share three electrons for a total of six shared electrons in the N 2 molecule Fig. In addition to elemental ions, there are polyatomic ions. It requires 8 electrons because that is the amount of electrons needed to fill a s - and p - orbital electron configuration ; also known as a noble gas configuration.

Each atom wants to become as stable as the noble gases that have their outer valence shell filled because noble gases have a charge of 0.

Although it is important to remember the "magic number", 8, note that there are many Octet rule exceptions. Example: As you can see from the picture below, Phosphorus has only 5 electrons in its outer shell bolded in red.

Argon has a total of 8 electrons bolded in red , which satisfies the Octet Rule. Phosphorus needs to gain 3 electrons to fulfill the Octet Rule. It wants to be like Argon who has a full outer valence shell. A single bond is when two electrons--one pair of electrons--are shared between two atoms.

It is depicted by a single line between the two atoms. Although this form of bond is weaker and has a smaller density than a double bond and a triple bond, it is the most stable because it has a lower level of reactivity meaning less vulnerability in losing electrons to atoms that want to steal electrons.

Below is a Lewis dot structure of Hydrogen Chloride demonstrating a single bond. As we can see from the picture below, Hydrogen Chloride has 1 Hydrogen atom and 1 Chlorine atom. Hydrogen has only 1 valence electron whereas Chlorine has 7 valence electrons.

To satisfy the Octet Rule, each atom gives out 1 electron to share with each other; thus making a single bond. A Double bond is when two atoms share two pairs of electrons with each other. It is depicted by two horizontal lines between two atoms in a molecule.

This type of bond is much stronger than a single bond, but less stable; this is due to its greater amount of reactivity compared to a single bond. Below is a Lewis dot structure of Carbon dioxide demonstrating a double bond. As you can see from the picture below, Carbon dioxide has a total of 1 Carbon atom and 2 Oxygen atoms. Each Oxygen atom has 6 valence electrons whereas the Carbon atom only has 4 valence electrons. To satisfy the Octet Rule, Carbon needs 4 more valence electrons.

Since each Oxygen atom has 3 lone pairs of electrons, they can each share 1 pair of electrons with Carbon; as a result, filling Carbon's outer valence shell Satisfying the Octet Rule. A Triple bond is when three pairs of electrons are shared between two atoms in a molecule. It is the least stable out of the three general types of covalent bonds. It is very vulnerable to electron thieves!