Metals, Nonmetals, and Movement of Electrons. Why Atoms Become Ions Noble gases have the most stable electron configuration of all atoms in a period.

Slides:

Advertisements

Similar presentations

Ions Atoms that are not neutral. Atoms Are Neutral Let’s review: Why are atoms neutral? –Because they have equal numbers of protons and electrons. Li.

Advertisements

Chemistry Homework Notes Read pp , problems pp. 165 #1-5, 10.

Atoms can attain a more stable arrangement of electrons in their outermost shell by interacting with one another. An ionic bond is formed when electrons.

IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence electrons.

6.1 Ionic Bonding.

An Introduction to Ionic Bonding Unit XX, Presentation 1.

Ch. 7: Ionic Compounds & Metals

The Periodic Table Periodic Properties.

Chemical Bonding.

2.4 Compounds, Atoms, and Ions

1 Chapter 4 Compounds and Their Bonds 4.1 Octet Rule and Ions Copyright © 2009 by Pearson Education, Inc.

The Periodic Table & Formation of Ions

Chapter 15 Ionic Bonding. Valence Electrons  Do the electron configuration for the following elements Li Be B O F Ne.

Objectives To describe the formation of ions from their parent atoms

Ions and Ionic Bonding. Electrons and Energy Levels First, let’s review: First, let’s review: Electrons are found in energy levels Electrons are found.

Science Olympiad. Science Fair Judges Recruit judges for the Science Fair Judges must be +21 years old Judges must have a background in science – College.

Ionic BONDING. Noble Gases Have complete outer shells that cannot accept anymore electrons Unreactive Will not combine (form bonds) with any other.

Chapter 8: Ionic Compounds P Section 8.1 Forming Chemical Bonds P

& Bell Work Write the Electron Configuration and Circle the Valence Electrons for: Magnesium Calcium.

Making Compounds. Chemical compounds form so that each atom has an octet of electrons in its valence level. This can occur by gaining, losing or sharing.

Electron Configuration and Bonding Section 15.1

Ionic Bonding Science 10 2 Keeping Track of Electrons The electrons responsible for the chemical properties of atoms are those in the outer energy level.

When you hear/see the word “ATOM” you can always assume that it is referring to the element in it’s NEUTRAL state A NEUTRAL ATOM means that there are.

Electron Configuration: Ions and Excite State. Electron Configuration - Cations  Cations – atoms that lose electrons - metals  Electron Configuration:

Notes: Ions Two ions are talking to each other in solution. One says: "Are you a cation or an anion?" The other replys, "Oh, I'm a cation." The first asks,

Positively charged ions and negatively charged ions are attracted to each other and this attraction is the basis of ionic bonding.

III. Periodic Trends. Types of Periodic Trends Atomic size (atomic radius) Ionic size (ionic radius) Ionization energy electronegativity.

Key Terms: Octet RuleIon CationAnion What is the difference between an atom and an ion? How can an atom become an ion? Why do chemists call table salt.

Number of ProtonsAtomic Number Number of NeutronsAtomic Mass – Atomic Number Number of ElectronsNumber of protons (Atomic Number)

 Monatomic ions consist of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons.

 Valence electrons: Electrons in the highest energy level  These electrons are the ones that bond!!  The group A # matches how many valence electrons.

 What is the electron configuration for Magnesium? What block, group and period does it belong to?  What is the noble gas configuration for Iodine? Is.

Notes: Ions 11/7 EQ: How do you find the ionic charge of an atom?

Unit 5: Ionic Bonding. 3s 2 3p 6 2s22s2 18-argon (Ar) 17-chlorine (Cl) 2s12s1 10-neon (Ne) 9-fluorine (F) Valence Electrons: e – ’s in highest energy.

Trends of the Periodic Table. Atomic radius - one half the distance between the nuclei of identical atoms that are bonded together.

Ionic Compounds Chapter 8 I will define a chemical bond I will describe how ions form I will identify ionic bonding and the characteristics of ionic compounds.

Midterm Review Chapter 5 & 6 Covalent and Ionic Bonding.

IONS. Neutral Atoms: Review Neutral Atoms have the same number of PROTONS and ELECTRONS. Protons have a POSITIVE charge. + Electrons have a NEGATIVE charge.

Ionic Bonds and Compounds. The Octet Rule The Octet rule states that elements gain or lose electrons to attain an electron configuration of the nearest.

Ionic Bonding. What makes an atom most stable? Electron configuration – Electron configuration – When the highest occupied energy level is filled with.

Valence Electrons  The number of electrons in the outermost energy level (shell) The currency of the atomic world Can be found from Bohr models/electron.

6.1 Ionic Bonding When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react. – The chemical.

Ions. Atoms are electrically neutral, that is, they have the same number of protons (+) as electrons (-). However, atoms are most stable when their valence.

Valence Electrons and Ions. Periodic Table of the Elements.

The Octet Rule. Happy atoms have a full outer energy level of electrons. They rarely combine with other elements. Nonreactivity is why they are called.

CHEMISTRY PART 4 Reactivity and Ions. Reactivity  Atoms want to be stable.  Want a full valence shell.  Want to be like the nearest Nobel Gas  The.

Ionization Energy What is “ionization energy”? Answer: the energy required to remove an electron from a gaseous atom This means that energy is required.

A n io n – negatively charged ion (more electrons than protons) Ex:  Fluorine has 9 e - and is reactive (7 e- in valence shell)  Adding one e - makes.

Atoms and Ions SNC2D. The Bohr-Rutherford Model Helium Atom 2 positive protons in nucleus 2 neutral neutrons in nucleus 2 negatively charged electrons.

..  Valence Electrons ◦ Electrons in highest energy level ◦ Largely responsible for chemical behavior (properties, bonding)  Noble gases have eight.

Vocabulary: 1. valence shell 2. valence electrons 3. anion 4. cation 5. isoelectric 6. Lewis structure (Lewis dot diagram) Banksy, British, 2002.

CHEMICAL BONDING the combining of atoms of elements to form new substances (compounds; two or more elements combined) Chemical bonding depends on the.

Science 10 Lesson 2 BOHR MODELS + IONIC BONDING. Student Review  Draw a model for sulfur atom.

Periodic Trends. Group Trends Group one, Alkali metals Group two, Alkaline earth metals Groups 3-12, Transition metals Group 17, Halogens Group 18, Noble.

Hydrogen and Helium Hydrogen does not share the same properties as the elements of group 1. Helium has the electron configuration of group 2 elements however.

When an atom gains or loses electrons they become electrically charged particles called When an atom gains or loses electrons they become electrically.

Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group? Do Now: Answer in your notebook If an atom.

Electron Configuration and Ion Formation

Lewis Structures and Ions

Ionic Bonding ..

Chp 5-1 Shell Models 1st shell (energy level): only 2 electrons

IONS Big Idea Atoms can gain or lose electrons to form charged particles called IONS.

PERIODIC TRENDS Chapter 6.

It’s time to talk about Bonds…

SCH3U-4C Matter & Qualitative Analysis

The Octet Rule.

Unit 1 – Atomic Structure

Periodic Trends Continued

Presentation transcript:

Metals, Nonmetals, and Movement of Electrons

Why Atoms Become Ions Noble gases have the most stable electron configuration of all atoms in a period. Atoms are more stable with full valence shells.

Metals Lose Electrons Metals have a low electronegativity (low ability to attract electrons) and a low ionization energy (easy to lose electrons). Metals will lose electrons to obtain a full valence shell like the noble gas in the period above them.

Nonmetals Gain Electrons Nonmetals have a high electronegativity (high ability to attract electrons) and a high ionization energy (hard to lose electrons). Nonmetals will gain electrons to obtain a full valence shell like the noble gas in the same period.

Forming Cations When a metal atom loses electrons, it no longer has a neutral charge. A charged atom is known as an ion. Cations refer to positively charged ions.

Forming Anions When a nonmetal atom gains electrons, it no longer has a neutral charge. Again, a charged atom is known as an ion. Anions refer to negatively charged ions.

Determining Ion Charge For metals in groups 1A, 2A, and 3A, the cation charge is equal to the number of valence electrons lost. For nonmetals, the anion charge is equal to the negative number of electrons gained. The charge sign is written to the right of the number.

Determining Ion Charge 1) What is the charge of the ion that forms from a nitrogen (N) atom? A)5+ B)3- C)3+ D)5-

Determining Ion Charge 2) What is the charge of the ion that forms from a magnesium (Mg) atom? A)2+ B)2- C)6+ D)6-

Determining Ion Charge 3) What is the charge of the ion that forms from a fluorine (F) atom? A)7+ B)7- C)1+ D)1-

Determining Ion Charge 4) What is the charge of the ion that forms from an aluminum (Al) atom? A)3- B)5+ C)3+ D)5-

Naming Monatomic Ions Group 1A, 2A, and 3A cations keep the name of the parent atom. Anions are named from the root of the nonmetal and add an “ide” ending.

Naming Monatomic Ions 5) What is the name of the Ba 2+ ion? A)barium B)baride C)boron

Naming Monatomic Ions 6) What is the name of the Cl 1- ion? A)chlorine B)chlorium C)chloride

Naming Monatomic Ions 7) What is the name of the ion that forms from a nitrogen atom? A)nitrogen B)nitride C)nitroxide

Naming Monatomic Ions 8) What is the name of the ion that forms from a potassium atom? A)potassium B)potasside C)potassygen