Covalent Bonding COVALENT BONDS occur when atoms electrons. When atoms combine through the sharing of electrons, are formed. What is a common example of a covalently bonded molecule? When hydrogen atoms bond covalently, they remain. Why do you think that is? H 2 gas is a double/single covalent bond. How many valence electrons do they share? Atoms forming covalent bonds try to obtain a outer electron shell. Using Lewis-dot models, show how H2O molecules are covalently bonded in the box below. - 1 pair of shared electrons between two - 2 pairs of shared electrons between two - 3 pairs of shared electrons between two In your model, what kind of bond exists between the oxygen atom and the hydrogen atoms? *there is no such thing has a quadruple bond!!!* Copy the structural formulas shown in the video in the space below. Each line in a structural formula represents a of shared electrons.
Covalent Bonding COVALENT BONDS occur when atoms share electrons. When atoms combine through the sharing of electrons, molecules are formed. What is a common example of a covalently bonded molecule? H2O (water) When hydrogen atoms bond covalently, they remain neutral. Why do you think that is? They never fully lose or gain electrons. H 2 gas is a double/single covalent bond. How many valence electrons do they share? 2 electrons (1 pair) Atoms forming covalent bonds try to obtain a stable outer electron shell. Using Lewis-dot models, show how H2O molecules are covalently bonded in the box below. - 1 pair of shared electrons between two atoms is called a single bond (2 total - 2 pairs of shared electrons between two atoms is called a double bond (4 total - 3 pairs of shared electrons between two atoms is called a triple bond (6 total In your model, what kind of bond exists between the oxygen atom and the hydrogen atoms? Two separate single bonds. *there is no such thing has a quadruple bond!!!* Copy the structural formulas shown in the video in the space below. Each line in a structural formula represents a pair of shared electrons.
Article from Thoughtco.com: Identifying Bond Types But, how do you know if a compound is ionic or covalent just by looking at a sample? This is where the properties of ionic and covalent compounds can be useful. Because there are exceptions, you need to look at several properties to determine whether a sample is ionic or covalent, but here are some characteristics to consider: Most crystals are ionic compounds. This is because the ions in these compounds tend to stack into crystal lattices to balance between the attractive forces between opposite ions and the repulsive forces between like ions. Covalent or molecular compounds can exist as crystals, though. Examples include sugar crystals and diamond. Ionic compounds tend to have higher melting and boiling points than covalent compounds. Ionic compounds tend to be hard and brittle while covalent compounds tend to be softer and more flexible. Ionic compounds conduct electricity when dissolved in water while covalent compounds typically don't. This is because covalent compounds dissolve into molecules while ionic compounds dissolve into ions, which can conduct charge. Information from: khanacademy.org All chemical bonding is due to electrostatic attraction. When atoms combine through chemical bonding, they form compounds unique structures composed of two or more atoms. The basic composition of a compound can be indicated using a chemical formula. A chemical formula uses symbols from the periodic table to indicate the types of elements present in a particular compound while using subscripts to represent the number of each type of element present.compounds can be covalent or ionic. In covalent compounds, atoms form covalent bonds that consist of electrons shared between two adjacent atomic nuclei. An example of a covalent compound is ammonia. The chemical formula of ammonia is NH3, which tells us that in a single molecule of ammonia, there is one nitrogen atom, and three hydrogen atoms. The structure of a covalent compound can be depicted through space-filling models as well as ball-and-stick models.in ionic compounds, electrons are completely transferred from one atom to another so that a cation positively charged ion and an anion negatively charged ion form. The strong electrostatic attraction between adjacent cations and anions is known as an ionic bond. The most common example of an ionic compound is sodium chloride NaCl, better known as table salt. Unlike covalent compounds, there is no such thing as a molecule of an ionic compound. This is because in nature NaCl does not exist in individual units, but in crystal lattice structures that are composed of multiple Na+ and Cl superscriptions alternating in space. The chemical formula NaCl specifies one formula
Using the information from the articles, organize the properties of ionic and molecular compounds below PROPERTIES OF IONIC COMPOUNDS PROPERTIES OF COVALENT MOLECULES Using the above information, fill in the venn diagram below IONIC COVALENT
Using the information from the articles, organize the properties of ionic and molecular compounds below PROPERTIES OF IONIC COMPOUNDS Form crystalline solids High melting points and boiling points Hard, brittle Conduct electricity when dissolved in water (conductivity) Involves ions Occurs between a metal and a nonmetal Shown with chemical formula Makes atoms more stable through the TRANSFER of valence electrons PROPERTIES OF COVALENT MOLECULES Can form crystalline solids (only sometimes) Low melting points and boiling points Soft, flexible Occurs between two nonmetals Shown with chemical formula Makes atoms more stable through the SHARING of valence electrons Uses prefixes when naming Using the above information, fill in the venn diagram below IONIC COVALENT -Form crystalline solids -High melting/boiling points -Hard, brittle -Conductive -Involves ions -Between a metal & nonmetal -TRANSFER of valence electrons -can form crystalline solids -shown with chemical formula -stable -Low melting/ boiling points -Soft, flexible -between two nonmetals -SHARING of valence electrons -Uses prefixes when naming