| A charged atom or molecule resulting from the loss or gain of one or more electrons. | Ion |
| What is an ion? | An ion is a charged atom or molecule. |
| A positively charged ion formed by the loss of one or more electrons from a metal atom. | Cation |
| What is a cation? | A positively charged ion resulting from the loss of electrons by a metal atom. |
| A negatively charged ion formed by the gain of one or more electrons by a non-metal atom. | Anion |
| What is an anion? | A negatively charged ion resulting from the gain of electrons by a non-metal atom. |
| A subatomic particle with a positive electrical charge, found in the nucleus of an atom. | Proton |
| What do positive cations have more of than electrons? | Positive cations have more protons than electrons. |
| A subatomic particle with a negative electrical charge, orbiting the nucleus of an atom. | Electron |
| What do negative anions have more of than protons? | Negative anions have more electrons than protons. |
| A stable configuration of electrons in an atom's outermost energy level, typically consisting of 2 electrons for the first shell and 8 electrons for subsequent shells. | Full Outer Shell |
| Why do atoms become ions? | Atoms become ions in order to achieve a full outer shell of electrons, which provides stability. |
| Forces of attraction that hold atoms together in a compound, resulting from the sharing or transfer of electrons between atoms. | Chemical Bonds |
| What are chemical bonds? | Forces of attraction that hold atoms together in a compound, arising from the sharing or transfer of electrons. |
| Chemical bonds formed by the transfer of electrons from one atom to another, typically between a metal and a non-metal. | Ionic Bonds |
| What type of atoms do ionic bonds typically form between? | Ionic bonds typically form between metal and non-metal atoms. |
| The process by which electrons are moved from one atom to another to form ions. | Electron Transfer |
| How do ionic bonds form? | Ionic bonds form when electrons are transferred between atoms. |
| A positively charged ion formed by the loss of electrons. | Cation |
| What is a cation? | A positively charged ion resulting from the loss of electrons by an atom. |
| A negatively charged ion formed by the gain of electrons. | Anion |
| What is an anion? | A negatively charged ion resulting from the gain of electrons by an atom. |
| Forces of attraction or repulsion between charged particles, such as ions. | Electrostatic Forces |
| What holds positive cations and negative anions together in an ionic bond? | Strong electrostatic forces. |
| A compound composed of positive and negative ions held together by electrostatic forces. | Ionic Compound |
| What results from the attraction between positive cations and negative anions in an ionic bond? | The formation of an ionic compound. |
| The method of determining the charge of an ion based on its position in the periodic table. | Ion Charge Prediction |
| How can the charge on an ion be predicted? | The charge on an ion can be predicted using the periodic table. |
| Elements in Group 1 of the periodic table, also known as alkali metals. | Group 1 Metals |
| What happens to the outer electron of Group 1 metals when they form ions? | Group 1 metals lose their 1 outer electron to form 1+ (positive) ions. |
| Elements in Group 2 of the periodic table, also known as alkaline earth metals. | Group 2 Metals |
| What happens to the outer electrons of Group 2 metals when they form ions? | Group 2 metals lose their 2 outer electrons to form 2+ (positive) ions. |
| Elements in Group 7 of the periodic table, also known as halogens. | Group 7 Non-metals |
| What happens to the outer electron of Group 7 non-metals when they form ions? | Group 7 non-metals gain 1 outer electron to form 1− (negative) ions. |
| Elements in Group 6 of the periodic table. | Group 6 Non-metals |
| What happens to the outer electrons of Group 6 non-metals when they form ions? | Group 6 non-metals gain 2 outer electrons to form 2− (negative) ions. |
| The electronic configuration of noble gases, characterized by a full outer shell of electrons. | Noble Gas Electronic Structure |
| What electronic structure do ions formed from Group 1, 2, 6, and 7 elements have? | They have the electronic structure of a noble gas, with full outer shells of electrons. |
| Compounds composed of positive and negative ions held together by electrostatic forces. | Ionic Compounds |
| Why do Group 1 and 2 metals form ionic compounds with Group 6 and 7 non-metals? | Because their ions have opposite charges, resulting in the formation of stable ionic compounds. |
| Diagrams representing the transfer or sharing of electrons between atoms in molecules or ions, using dots to represent electrons from one atom and crosses to represent electrons from another atom. | Dot and Cross Diagrams |
| What do dot and cross diagrams illustrate? | Dot and cross diagrams illustrate the transfer or sharing of electrons between atoms in molecules or ions. |
| An atom of sodium, typically represented in dot and cross diagrams by dots to denote its valence electrons. | Sodium Atom |
| How are electrons from a sodium atom represented in dot and cross diagrams? | They are represented by dots. |
| An atom of chlorine, typically represented in dot and cross diagrams by crosses to denote its valence electrons. | Chlorine Atom |
| How are electrons from a chlorine atom represented in dot and cross diagrams? | They are represented by crosses. |
| Compounds formed by the electrostatic attraction between positive and negative ions. | Ionic Compounds |
| What do dot and cross diagrams illustrate about the formation of ionic compounds? | They illustrate how electrons are transferred between atoms to form ions, which then combine to form ionic compounds. |
| A positively charged ion formed by the loss of an electron from a sodium atom. | Sodium Ion |
| What type of ion does a sodium atom become in the formation of an ionic compound (NaCl)? | A positively charged sodium ion (Na+). |
| A negatively charged ion formed by the gain of an electron by a chlorine atom. | Chloride Ion |
| What type of ion does a chlorine atom become in the formation of an ionic compound (NaCl)? | A negatively charged chloride ion (Cl-). |
| Dot and cross diagrams that only represent the outer (valence) electrons of atoms involved in bonding. | Simplified Dot and Cross Diagrams |
| How are dot and cross diagrams sometimes simplified? | They are simplified by only showing the outer electrons of atoms involved in bonding. |
| The process by which electrons are moved from one atom to another, resulting in the formation of ions. | Electron Transfer |
| What is electron transfer? | Electron transfer is the movement of electrons from one atom to another. |
| A compound formed by the combination of magnesium and chlorine atoms, typically in a 1:2 ratio. | Magnesium Chloride |
| What compound is formed when magnesium reacts with chlorine? | Magnesium chloride. |
| An atom of magnesium, typically represented with its two outer electrons in dot and cross diagrams. | Magnesium Atom |
| How many electrons does a magnesium atom have in its outer shell? | A magnesium atom has 2 electrons in its outer shell. |
| A positively charged ion formed by the loss of electrons from a magnesium atom. | Magnesium Ion |
| What type of ion does a magnesium atom become in the formation of magnesium chloride? | A magnesium ion (Mg2+). |
| An atom of chlorine, typically represented with its seven outer electrons in dot and cross diagrams. | Chlorine Atom |
| How many electrons does a chlorine atom need to gain to achieve a full outer shell? | A chlorine atom needs to gain 1 electron to achieve a full outer shell. |
| A negatively charged ion formed by the gain of electrons by a chlorine atom. | Chloride Ion |
| What type of ion do chlorine atoms become in the formation of magnesium chloride? | Chloride ions (Cl-). |
| The principle that the total charge before and after a chemical reaction remains constant. | Charge Conservation |
| How do the charges of magnesium and chloride ions in magnesium chloride relate to the electron transfer process? | The magnesium ion has a 2+ charge because it loses 2 electrons, while each chloride ion has a 1- charge because they each gain 1 electron, ensuring charge conservation. |
| The number of protons in the nucleus of an atom, denoted by the symbol Z. | Atomic Number |
| What does the atomic number represent? | The number of protons in the nucleus of an atom. |
| The total number of protons and neutrons in the nucleus of an atom, denoted by the symbol A. | Mass Number |
| What does the mass number represent? | The total number of protons and neutrons in the nucleus of an atom. |
| A subatomic particle with no electrical charge, found in the nucleus of an atom. | Neutron |
| How can the number of neutrons in an atom be determined? | By subtracting the atomic number from the mass number. |
| An atom of lithium, typically containing 3 protons, 4 neutrons, and 3 electrons. | Lithium Atom |
| How many protons does a lithium atom have? | 3 protons. |
| A positively charged ion formed by the loss of one electron from a lithium atom. | Lithium Ion (Li+) |
| What happens to a lithium atom when it becomes a lithium ion? | It loses one electron, resulting in a positive charge (Li+). |
| The principle that the total charge before and after a chemical reaction remains constant. | Charge Conservation |
| How is the number of electrons in a lithium ion calculated? | By subtracting the number of electrons lost from the number of electrons in the neutral lithium atom. (3 − 1 = 2) |
| The arrangement of electrons in the orbitals of an atom or ion. | Electron Configuration |
| What is the electron configuration of a lithium ion (Li+)? | 2 electrons, as it loses 1 electron to become positively charged. |
