Untitled Flashcards Set

Dot Diagrams

diagrams that represent the valence electrons of an atom as dots around the element's symbol.

Valence electrons: are the electrons in the outermost shell of an atom and are crucial for chemical bonding.

• Lewis Structures: These are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist.

• Structural Formulas: These show the arrangement of atoms within a molecule.

• Ionic Bonds: These bonds form when one atom transfers one or more electrons to another atom, resulting in the formation of positively charged cations and negatively charged anions.

• Covalent Bonds: These bonds form when atoms share electrons to achieve a full outer shell.

• • Polar Covalent Bonds: These occur when electrons are shared unequally between atoms, creating a dipole.

  • Non-Polar Covalent Bonds: These occur when electrons are shared equally between atoms.

• Ionic Compounds: These are composed of cations and anions held together by ionic bonds.

• Covalent Compounds: These are composed of molecules held together by covalent bonds. They typically form between non-metals.

• Acids and Bases: Acids are substances that donate protons (H⁺ ions), while bases are substances that accept protons. Example: Hydrochloric Acid (HCl) is an acid, and Sodium Hydroxide (NaOH) is a base.

• all metal properties are: Malleable, Ductile,Conductivity and Luster

• Luster: Metals have a shiny appearance due to their ability to reflect light.

• Malleable: Metals can be hammered or rolled into thin sheets without breaking.

• Ductile: Metals can be drawn into wires without breaking.

• Conductivity: Metals are good conductors of heat and electricity due to the free movement of electrons.

• Formula Unit: The simplest ratio of ions in an ionic compound.

• Diatomic Molecules: These are molecules composed of two atoms of the same element.

all diatomic molecules:H2 N2 O2 F2 Cl2 Br2 I2

• Transition Metals with Multiple Charges: These metals can form ions with different charges.

• Particles to Moles: Use Avogadro's number (6.022 x 10²³ particles/mol) to convert the number of particles to moles. For example, 1 mole of any substance contains 6.022 x 10²³ particles.

• Anion: A negatively charged ion formed by gaining electrons. Example: Cl⁻.

• Cation: A positively charged ion formed by losing electrons. Example: Na⁺.

• Molecule: A group of atoms bonded together, representing the smallest fundamental unit of a chemical compound.

• Chemical Formula: A representation of the elements in a compound and their ratios.