Chem

• Metallic bonds are formed between metal atoms, where the valence electrons are delocalized and free to move throughout the structure.
• Ionic compounds form from metals that lose electrons (cations) and non-metals that gain electrons (anions).
• Covalent bonds are formed when two atoms share one or more pairs of electrons to achieve a full outer shell, resulting in a stable molecule with no net charge on either atom.
• Hydrogen bonding is a type of intermolecular force that occurs between hydrogen atoms covalently bound to highly electronegative elements such as fluorine, oxygen, nitrogen, and sulfur.
• Metallic bonds have a high melting/boiling point, are hard and malleable and are conductive in all phases.
• Covalent bonds have a low boiling/melting point, are soft and brittle, and are non-conductive in all states.
• Ionic bonds have high boiling/melting points, are hard and brittle and are conductive in all states besides solid.
• Metal bonds contain mobile electrons, making them constantly moving and easy to conduct through.
• Ionic bond = metal ion + nonmetal ion together :) a metal TRANSFERS or DONATES its valence electrons to a non metal
• Covalent compound (also known as molecules or molecular compound) is two nonmetals that SHARE their valence electrons. they do this because neither are electronegative enough (attractive to electrons) to take away valence electrons
• Metallic bonds are bonds only between metal elements. Valence electrons are mobile and/or moving around atoms, this is why they’re good conductors of electricity.
• Metallic bonds are also described as a “sea of electrons.”
• Electronegativity is the measure of how polar electrons are to each other (how good they are at attractive each other)
• Nonmetals are highly electronegative. They receive electrons way more than metals which give up their electrons.
• Metalloids on the periodic table include the staircase starting at b, se, ge, as, sb, te, and at. From the right side of that all are non metals. Those to the left of the staircase are metals excluding hydrogen (non metal)
• To name an ionic compound, you firstly have to look at the positive charges listed. If the ion has Only one positive charge listed, it’s the same as its element name. If two or more are named, the charge is listed after the element name in parenthese.
• To name a non metal anion, you take the name of the element of a non metal and take off the ending of the non metal element and add the ide. (Ex, chlorine becoming chloride)
• The metals/cations always come first
• you can find out if a MOLECULE is polar or non-polar by looking at its symmetry. If it has only one line, it’s polar. If it has more than one, it’s non polar.
• You can tell if a BOND is polar or non-polar by looking at the difference between the electronegativity of two elements in the bond. Less than .5= non-polar, more than .5 is polar
• As temperature increases in table h, vapor pressure also increases.
• As vapor pressure increases, there are more gas molecules, and if there are more gas molecules the liquid has a weaker intermolecular force and the molecules do not remain liquid.
• The easier it is to get a liquid to its boiling point, the weaker its Intermolecular forces are.