Elements and compounds are pure chemical substances found in nature. The difference between an element and a compound is that an element is a substance made of same type of atoms, whereas a compound is made of different elements in definite proportions.Examples of elements include iron, copper, hydrogen and oxygen.Examples of compounds include water (H 2 O) and salt (Sodium. How elements relate to atoms. The basics of how protons, electrons and neutrons make up an atom.Watch the next lesson: https://www.khanacademy.org/science/ch.

1. Atoms Elements And Compounds Bbc Bitesize
2. Atoms Elements And Compounds Powerpoint

Atoms, Elements, and Compounds.    Lesson 6:  Ionic & covalent compounds. Activo laptops & desktops driver download for windows 10. Powered by Create your own unique website with customizable templates. Worksheet:compounds are when two or more elements combine. Chemistry is the study of matter. Atoms, Elements, and Compounds! Atoms are the building blocks of matter. Section 1 Chemistry in Biology! Neutrons and protons are located at the center of the atom.! Protons are positively charged particles.! Neutrons are particles that have no charge.

Simple distillation is a method for separating the solvent from a solution, leaving behind the solute. This method works because the solvent has a much lower boiling point than the dissolved solute. Heating the solution allows the solvent to evaporate, and then it passes through a condenser, where it is cooled and condensed into a separate container. The solute does not evaporate and so it stays behind.

Fractional distillation is a method of separating multiple liquids from each other. The technique works in the same way as distillation, but on a much larger scale.

Atoms Elements And Compounds Bbc Bitesize

Filtration is a method for separating an insoluble solid from a liquid. A mixture of liquid and solid is passed through filter paper into a flask below. The solid stays on the filter paper (residue), and the liquid passes through to the container below (filtrate).

Crystallisation/evaporation is a method that separates a soluble solid from a liquid. A solution of liquid and dissolved solid is heated, causing the solvent to evaporate and leaves solid crystals behind.

Atomic Theory

Atomic theory first got discovered by scientists who each had different theories. The scientist known as Dalton was the one who had suggested “that matter is made up of atoms”, which was then found as true. Thomson said that ” atoms contain negatively charged particles” which we now call electrons; that was also found later as true. The scientist Rutherford discovered that “the nucleus and ti’s subatomic particles” he thought that the nucleus was made up of positively charged particles. Later known as protons and particles with nob charge were later called neutrons. Bohr then came along and said that “electrons are located in shells which are found around the nucleus”. With all of there discoveries the atomic theory was studied and created.

The Atom

The difference between atoms and molecules are that molecules can gain or lose one or more electrons, while atoms combine to form molecules.

Electrons: are found in the shells, and have a negative charge.

Protons: are found in the nucleus, and have a positive charge.

Neutrons: are found in the nucleus, and have no/neutral charge.

The atomic number on the periodic table of elements represents the amount of protons are in the nucleus. The atomic mass is the mass of the element. Groups are horizontal, and they represent the same properties. Families are vertical and they represent the same number of valence electrons.

The differences between metals, non-metals, and metalloids,are metals are shiny,conductors, and have high density. Non-metals are dull, poor conductors and low density. Metalloids can be shiny or dull, and can conduct better than non-metals but not as well as metals.

Alkali Metals

All the alkali metals react vigorously or explosively with cold water, producing an aqueous solution of the strongly basic alkali metal hydroxide and releasing hydrogen gas.This reaction becomes more vigorous going down the group: lithium reacts steadily with effervescence, but sodium and potassium can ignite and rubidium and caesium sink in water and generate hydrogen gas so rapidly that shock waves form in the water that may shatter glass containers When an alkali metal is dropped into water, it produces an explosion, of which there are two separate stages. The metal reacts with the water first, breaking the hydrogen bonds in the water and producing hydrogen gas; this takes place faster for the more reactive heavier alkali metals. Second, the heat generated by the first part of the reaction often ignites the hydrogen gas, causing it to burn explosively into the surrounding air. This secondary hydrogen gas explosion produces the visible flame above the bowl of water, lake or other body of water, not the initial reaction of the metal with water (which tends to happen mostly under water).

Alkaline Earth Metals

The alkaline earth metals all react with the halogens to form ionic halides, such as calcium chloride as well as reacting with oxygen to form oxides such as strontium oxide. Calcium, strontium, and barium react with water to produce hydrogen gas and their respective hydroxides.

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Fluorine reacts vigorously with water to produce oxygen and hydrogen fluoride Dissolved chlorine reacts to form hydrochloric acid a solution that can be used as a disinfectant or bleach. Bomine slowly reacts to form hydrogen bromide and hypobromous acid. Iodine However, iodine will form an aqueous solution in the presence of iodide ion, such as by addition of potassium iodide because the triiodideion is formed.

Noble Gases

The noble gases are usually inert, because their electron shells are full. The further away an electron is the higher its energy and the less of a hold the protons have one it. If a highly electro-negative element comes in contact with a noble gas in high heat, the noble gas can lose an electron. The noble gas becomes a cation. The cation noble gas is free to from a ionic bond with a anion.

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A substance consisting of atoms which all have the same number of protons (the same atomic number). Elements are chemically the simplest substances and hence cannot be broken down further using chemical methods. Elements can only be changed into other elements using nuclear methods. A chemical element is a substance that cannot be broken down by chemical means. Elements are defined by the number of protons they possess. Examples of Elements include:copper, cesium, iron, neon

Compounds

A compound is a chemical species that is formed when two or more atoms join together chemically, with covalent or ionicbonds. Also Known As: molecule, though sometimes distinctions are made between the types of bonds in molecules (covalent) and compounds (ionic)

An atom that has an equal number of protons and electrons isn’t positive or negative, it has no charge. If that atom gains or loses electrons it may become a cation, an ion with a positive charge, or an anion, an ion with a negative charge. Chemists use a very simple way to represent ions in chemical reactions. Remember some common polyatomic ions amd you can figure out the symbols for ions just using the periodic table of elements.

Atoms

An atom is the defining structure of an element. Elemental atoms differ from each other by the number of protons in their nucleus. For example, one way to tell oxygen atoms from nitrogen atoms would be to count the number of protons each atom has. Oxygen will have eight where nitrogen will have seven. Stable atoms have the same number of electrons as the number of protons. These electrons form orbitals around the nucleus and cause much of the chemical properties of the element. When an atom’s outermost orbital gains or loses electrons (also known as valence electrons), the atom forms an ion.

Ions: Ions are atoms or molecules that have gained or lost one or more of their valence electrons and have a net positive or negative charge.

Naming

Non-metals & Metals

Sodium bromide — NaBr
Magnesium oxide — MgO
Zinc fluoride — ZnF₂

• Multivalent Metals

Iron (III) oxide — Fe₂O₃
Tin (II) fluoride — SnF₂
Copper (I) chloride — CuCl

• Polyatomic Ions

Sodium bicarbonate — NaHCO₃
Calcium nitrate — Ca(NO₃)₂
Ammonium hydroxide — NH₄OH
Lithium nitrate — Li₂Cr₂O₇

Formula to name

• Non-metals & Metals

CaCl₂ — Calcium chloride
ZnS — Zinc sulphide
Na₃N — Sodium nitride

• Multivalent Metals

PbO₂ — Lead (IV) oxide
SnH₄ — Tin (IV) hydride
CrS — Chromium (II) sulphide

• Polyatomic Ions

Pb(CIO₃)₂ — Lead (II) chlorate
H₂SO₄ — Hydrogen sulphate
Fe₂(SO₄)₃ — Iron (III) sulphate
Cu₃(PO₄)₂ — Copper (II) phosphate

Properties of Matter

Mass: The amount of matter within an object.
Volume: The amount of space an object takes up.
Density: How much mass in a specific volume an object has.
State: What state an object is in; liquid, solid, or gas.
Colour: The colour of an object.
Melting Point: The temperature where a solid turns into a liquid.
Boiling Point: The temperature where a liquid turns into a gas.
Conductivitiy: The ability of an object to let heat or electricity flow.

Physical & Chemical Changes

Physical and chemical changes are different in what results from each.

Physical Changes

• Melting
• Ripping
• Cutting
• Grinding
• Tearing
• Dissolving

Chemical Changes

• Colour change
• Heat
• Light
• Sound
• Bubbles

State Change & the Kinetic Molecular Theory

Matter exists in three states, solid, liquid, and gas.

Solid: The particles are very tightly packed, and they have no space to move. They vibrate in place.
Liquid: The particles have a bit more space to move, so they slide past each other.
Gas: The particles have a lot of space to move, and they move freely.

Atoms Elements And Compounds Powerpoint