Periodic Table Vocab & Concepts PDF

# Periodic Table Vocab - The columns of the periodic table are called **GROUPS**. - The rows of the periodic table are called **PERIODS**. - Electrons are located in **ENERGY LEVELS** around the nucleus. - **Valence Electrons** are the electrons located in the outermost energy level of an atom. - T...

# Periodic Table Vocab - The columns of the periodic table are called **GROUPS**. - The rows of the periodic table are called **PERIODS**. - Electrons are located in **ENERGY LEVELS** around the nucleus. - **Valence Electrons** are the electrons located in the outermost energy level of an atom. - The number of valence electrons in an atom influences the chemical properties of an element. ## Bonds - **Atomic Radius** - a measure of the distance from the center of the nucleus to the outermost energy level. - Decreases as you move across a period. - **Ionisation Energy** - the amount of energy it takes to remove one valence electron from an atom. - Higher ionisation energy means the atom is less likely to lose electrons. - Stronger magnetization, more energy is needed. - **Electronegativity** - a measure of how strongly an atom attracts a pair of electrons to itself when bonded with another atom. - The more strongly an atom can attract bonded electrons, the higher the value. - Fluorine, F, is most electronegative. - Increases as you move across a period and from bottom to top in a group. ## Sonic Radius - The radius changes for an atom when it forms ions. - Positive ions (Cations) lose one or more valence electrons. - Radius shrinks as you move across a period and shrink as you move from bottom to top. - Negative ions (Anions) gain one or more valence electrons. - Radius increases as you move across a period and increase as you move from bottom to top. # Families of Periodic Table ## Alkali Metals and Hydrogen - Group 1 or 1A - H, Li, Na, K, Rb, Cs, Fr - First group - Hydrogen is not an alkali metal, but it has similar properties. - Soft metals that are very reactive with water and have low melting points. ## Alkaline Earth Metals - Group 2A - Be, Mg, Ca, Sr, Ba, Ra - Second group. - Less reactive than Group 1A. - Radium is radioactive. ## Transition Metals - Groups 3-12. - Typical metals that are still reactive. - Dissolves in water, forming colored solutions. ## Metalloids - Found on either side of the stair-step line. - Have properties of both metals and non-metals. - Often used as semiconductors. ## Chalcogens (Oxygen Family Group) - Group 6A or 16. - Become more metallic as you move down a column. - O, S, Se, Te, Po, Lv ## Halogens - Group 7A or 17. - Means "Salt-Former". - Readily react with Group 1 & 2 to form salt compounds. - One electron short of having a full valence shell. - Extremely reactive. - F, Cl, Br, I, At ## Noble Gases - Group 8A, 18. - Chemically inert (Unreactive gases). - Some can react under the right conditions to form compounds. - He, Ne, Ar, Kr, Xe, Rn # Metal? Jab Analysis 1. **Conductive and malleable** - Al, Fe, Sn, Zn. 2. **Not conductive and brittle** - C, SE. 3. **Either/Neither** - Si. 4. **Metal** - Al, Fe, Sn, Zn 5. **Non-metal'' - C, S. 6. **Metalloid** - Si. 7. **Se** - Probably doesn't react with acid or copper(II) chloride solution. 8. **Ca** - Probably reacts with acid or copper(II) chloride solution. 9. **Co** - Probably reacts with acid or copper(II) chloride solution. # Electron Configuration - **Orbital Electron Cloud**: 90% chance to find an electron in a region of space where there is a higher probability of finding an electron. - **Noble Gas Notation**: A shorthand method for showing the electron configuration of an atom. - **Energy Level**: 1s2 2s2 2p6. - The largest number represents the energy level. - The letters represent the orbitals. - The superscripts represent the number of electrons in each orbital. - **Valence Electrons**: The electrons in the outermost energy level. They are involved in chemical bonding. Total number of valence electrons - 8. # Parts of an Atom, Atomic Number, Atomic Mass - **Subatomic particles:** - **Proton** - Positively charged particle. - **Neutron** - No charge particle. - **Electron** - Negatively charged particle. - **Nucleus** - Contains protons and neutrons. - Almost all mass of an atom comes from here. - **Atomic Number** - The number of protons in the nucleus of an atom. - An atom is neutral when the number of protons equals the number of electrons. - **Atomic Mass** - The average mass of all the isotopes of an atom. - **Isotopes** - Atoms with the same number of protons but different numbers of neutrons. - They have similar chemical properties, but their physical properties can differ. - **Nuclear Notation** - A = Z + N - A = Atomic mass. - Z = Atomic number. - N = Number of neutrons. # Ions and Isotopes - **Ions** - Atoms that have gained or lost electrons. - **Cation** - Formed when an atom *loses* electrons. - **Anion** - Formed when an atom *gains* electrons. # Electromagnetic Radiation - One of the ways that energy travels. - **Wavelength** - The distance between two peaks or troughs of a wave. - **Frequency** - The number of waves per second that pass a given point. - **Planck's Constant** - A fundamental constant represented by h (6.62607015 *10^-34) Joule second. - **Dual Nature of Light** - Light can behave like both a wave and a particle. - It exists in packets of energy known as **quanta**. - **Excited State** - Atom with excess energy. - **Ground State** - An atom in its lowest possible energy state. - **Energy Level Diagram** - A diagram that shows the different energy levels of an atom and the transitions between them. # Types of Ions - **Monatomic Ions** - Only one element involved. - **Polyatomic Ions** - Multiple elements involved. - Example: OH-, NO3-, HCO3-, CO3 2-, SO4 2-, PO4 3-