Atoms, Ions, Molecules and Polarity

Slides:



Advertisements
Similar presentations
Atoms Chapter 2, Section 1.
Advertisements

CH. 2 Chemistry of life Section 1 Nature of matter
CHEMISTRY.
Biochemistry 2.1. Matter Chemical changes in matter are essential to all life processes. Matter: Anything that occupies space and has mass. Mass: The.
Early Chemistry  Early Chemists only believed in 1 element: Dirt  Later Chemists believed in 4 elements: Air Earth Fire Water  Various combinations.
What you should learn: How compounds differ from the elements that make them How a chemical formula represent the ratio of atoms in a compound How the.
ESCS Review. Composition of Matter (Review) Matter – anything that takes up space and has mass. Mass – the quantity of matter an object has (the same.
Atoms and Molecules Atom is smallest particle that can be identified as a particular substance. Molecule is two or more atoms bonded to each other.
Chapter 4- Earth Chemistry
Chapter 2~The Chemistry of Life
Class Starter Look at the different substances and write down which substances you think are composed of elements and which are composed of compounds.
What Makes Up Matter?. Atom- Small particle that makes up types of matter. Law of Conservation of Matter- Matter is not created or destroyed… it only.
Chapter 2.1.  Why do we care about chemistry in Earth Science?  The earth is made up of rocks and minerals.  Rocks and minerals are made of elements.
The Chemical Compounds of Life Basic chemistry. Matter Anything that has mass and takes up space is matter. There are about 103 naturally occurring different.
Atoms, Elements, & Compounds Biology II D. Mitchell.
Chemical Bonding. Matter and Mass  Anything that a mass and takes up space has matter.  The mass of an object is how much matter you have.  Mass is.
CHEMISTRY IN LIVING SYSTEMS. All life processes involve living things made of matter All matter is composed of elements The chemical foundation for the.
The Chemical Context of Life
Section 1: Atoms, Elements, and Compounds
Chapter 2: The Chemistry of Life
Nature of Matter. Atom smallest unit of matter that cannot be broken down by chemical means.
Matter & Atoms Unit 2. Matter Matter – anything that has mass and takes up space. Matter is made up of MUCH smaller particles known as atoms. 1)
Matter Chapter 2, Section 1. Elements and the Periodic Table Element – a substance that cannot be broken down into simpler substances by ordinary chemical.
 Atoms are the smallest form of matter  Nucleus: ◦ Protons (positive) ◦ Neutrons (neutral) ◦ Protons & neutrons make up most of the atom’s mass  Energy.
 The atomic number equals the number of protons.  The electrons in a neutral atom equal the number of protons.  The mass number equals the sum of.
The Chemistry of Life The Nature of Matter Chemistry- The study of matter Matter- Anything that takes up space and has mass. Mass- A measure of the amount.
Chapter 6.1 Biology. Intro to the Chemistry Your life DEPENDS on chemistry! 1.When you inhale oxygen, your body uses it in chemical reactions! 2.When.
THE CHEMISTRY OF LIFE The Nature of Matter. What do all of These Pictures Have in Common?
BELL-RINGER QUESTION 1. Look at the periodic table of elements…. How are the elements in the periodic table like the alphabet of letters?
CH2 Sec1 Matter and Substances. Everything is made up of matter. Matter is anything that has mass and takes up space.
Chemistry of Atoms Chapter 4 Weekly Objectives All organisms are made of cells, and all cells are made of chemical substances, including water, carbohydrates,
Ch. 8 Earth Chemistry. Journal: What do we know about matter?
CHAPTER 2 COMPOSITION OF MATTER MATTER- anything that occupies space and has mass MASS- quantity of matter an object has ELEMENT- a pure substance that.
The Chemistry of Life Atoms and Elements Chapter 6.
Chemistry Review. Proton positively charged part of an atom –found in the nucleus –has mass –constant in every atom of an element Ex: every atom of oxygen.
Minerals – Chemistry Review. Minerals are made up of different chemical elements bound together.
Introduction to Chemistry Unit D Chapter 1.1 NCSCOS 4.01 and 4.02.
Review for the Physical Science Final By Samantha Pereira.
EQ: What are the two types of chemical bonds and what makes each one unique?
1.4 Chemistry Basics Part I SBI3C Mrs. Jones. Chemistry Basics  Biology is the study of living things  All living matter is composed of chemical substances.
Matter, Atoms, Elements A chemistry review. What’s matter?  Matter is anything that has mass and volume  Mass is  Volume is  Matter is made up of.
What you’ve learned so far…..  Atoms form bonds in more than one way  In IONIC bonding, atoms give up or gain electrons  In COVALENT bonding, atoms.
Chemistry Notes: Atomic Structure. What is matter? Matter is anything that has mass and volume. It can be a solid, liquid, or gas.
Ch. 11 Section 1 Review Development of the Atomic Theory.
BASIC CHEMISTRY Becky Sheridan. What is stuff made of? Matter: –Occupies space & has mass Elements: –Pure chem. substance that can’t be broken into other.
The Chemistry of Life Or Biochemistry Atoms, Molecules, Compounds, Chemical Bonds.
ChemistryChemistry. Early Chemistry Dirt  Early Chemists only believed in 1 element: Dirt 4 elements  Later Chemists believed in 4 elements: Air Earth.
BASIC CHEMISTRY I thought this was biology? Objective: 1.To Understand what causes chemical bonds 2.To be able to read an equation 3.To Understand polarity.
Section Objectives: Relate the structure of an atom to the identity of elements. Relate the formation of covalent and ionic chemical bonds to the stability.
Early Chemistry Early Chemists only believed in 1 element: Dirt
Early Chemistry.
Chapter 1: The Chemistry of Life
Chemistry.
Early Chemistry Early Chemists only believed in 1 element: Dirt
2.1 – Matter all objects are made of matter
Matter & Atomic Structure
Atoms Atomic Structure.
Early Chemistry Early Chemists only believed in 1 element: Dirt
Characteristics of Life Part 2: Chemistry of Life
Chapter 20 Section 2: Types of Bonds
Nature of Matter.
Chemistry of Life Chapter 2.
Self Quiz.
Matter & Atomic Structure
Chemistry Basics.
The Chemistry of Biology
10T2K© Atoms and bonds.
The Chemical Basis of Life
Chemical Bonds 18.2.
Covalent Bonding.
Presentation transcript:

Atoms, Ions, Molecules and Polarity Basic Chemistry Atoms, Ions, Molecules and Polarity

Introduction Chemistry is the central science, meaning that all other science are based on chemistry. Why? Because chemistry is the study of matter and energy…specifically the atom

Building Blocks We will learn that in biology, the building block of life is the cell. In chemistry however, the building block of all matter is the atom.

Structure of the Atom For many years the atom was thought to be the smallest particle and that it could not be divided into anything smaller. Now we know that atoms are not the smallest particles. In fact, atoms are made of subatomic particles known as: Protons Neutrons Electrons

General Structure There are two parts to the atom Nucleus A very small area in the center of the atom that contains most of the mass. The locations where protons and neutrons are found. Electron Cloud The area of the electron that takes up the most space. The location where the electrons are found.

Subatomic Particles Protons The second largest particle in the atom The number of protons determines the identity of the atom Located in the nucleus Has a positive charge Charge means that an object has an attraction to some objects and is repelled by another. In this case the proton is attracted to negatively charged particles.

Subatomic Particles Neutrons The largest particle in the atom The number of neutrons in an atom greatly impacts the mass of the atom. Located in the nucleus Has a neutral charge Charge means that an object has an attraction to some objects and is repelled by another. In this case the neutron has no charge and therefore does not attract any other particles.

Subatomic Particles Electrons The smallest of the three major particles The interaction of electrons give the atom it’s characteristics Located in the electron cloud Has a negativecharge Charge means that an object has an attraction to some objects and is repelled by another. In this case the electron has a negative charge and attracts positively charged particles.

Neutral Atoms Atoms typically have the same number of protons and electrons making them neutral. Just as with the neutrons, when a substance is neutral there is not attraction to another particle. If atoms always stayed neutral, there would be no interaction between atoms and the world would be left with about 92 different objects only instead of the trillion or more that exist today.

Ions The electrons determine the characteristics of the atom. Thus the interaction between atoms to form compounds is a result of the interaction between electrons. In the process of interacting atoms sometimes gain or lose electrons in the process forming ions.

Formation of Ions: Losing Electrons A large group of elements wants to lose electrons. This group is called the metals. When a element loses electrons the overall charge on the atom becomes positive. This is because the atom now has more positives than negatives. Protons can NEVER be gained or lost so gaining and losing electrons is the only way to change the charge on the normally neutral atom.

Formations of Ions Gaining electrons A smaller group of elements wants to gain electrons. This group is called the non-metals.

Formation of Ions: Gaining Electrons Losing electrons A smaller group of elements wants to lose electrons. This group is called the non-metals. When a element gains electrons the overall charge on the atom becomes negative. This is because the atom now has more negativesthan positives. Protons can NEVER be gained or lost so gaining and losing electrons is the only way to change the charge on the normally neutral atom.

Ion Formation and Bonding The ability of an atom to gain or lose electrons allows that atom to interact, or bond, with another atom to form a completely new substance.

Bonding There are two types of bonding that can occur Ionic bonding Caused by the transfer of electrons from one atom to another Covalent bonding Caused by the sharing of electrons between different atoms.

Ionic Bonding In ionic bonds, ions are formed creating two oppositely charged particles. One or more atoms transfers their electron to another atom. The atom that does the transferring loses electrons and becomes positive. The atom that does the receiving gains electrons and becomes negative. The attraction between the two charged particles results in a compound being formed. This compound has very different properties than the elements involved in the formation.

Covalent Bonding In covalent bonding, nonmetal elements share their electrons. When electrons are shared between atoms they interact forming a new compound. This compound usually has very different properties than the elements that are bonded together.

Unequal Sharing When atoms share electrons, there are two different ways in which they can be shared Equally These form non-polar molecules Unequally These form polar molecules

Non-Polar Bonds Polarity is determined by the location of the electrons between two atoms. When atoms share the electrons equally, the electrons spend as much time with one atom as they do another essentially seeming as if they are in the middle.

Polar Bonds When atoms share the electrons unequally, the electrons spend more time with near the nucleus of one atom than the other, essentially seeming as if it were at one pole or another. Imagine the poles of the earth. They are located at one extreme or the other. This is how the electrons in this type of bond can be pictured.