Particle Nature of Matter PDF

Reviewer.docx 1/3 Particle Nature of Matter Matter – is anything which occupy space and has weight. Properties – characteristics that describe a sample of matter. Mass – a measure of the amount of matter the object has. Volume – measure of the space occupied by an object. Other particles of m...

Reviewer.docx 1/3 Particle Nature of Matter Matter – is anything which occupy space and has weight. Properties – characteristics that describe a sample of matter. Mass – a measure of the amount of matter the object has. Volume – measure of the space occupied by an object. Other particles of matter: 1. Hardness 2. Texture 3. Color 4. Flexibility 5. Malleability 6. Electrical conductivity Solid - have definite shapes and volume because the particles are packed tightly. - vibrating in place. Liquid - Are closer to one another, pressing one another as they move. Gas - Takes the shape of the container. Particle model of matter – shows that in gases, the particles move at random directions very quickly and Travel in straight-line paths. Density - describes how much space an object or substance takes up. - the amount of mass per unit volume. Physical Changes of Matter Physical Change – is a change in which no new material forms. Substances – are capable of changing their physical phase when the conditions are altered. Temperature – conditions that make substances transform from one phase to another. Evaporation – the process by which the molecules on the surface of a liquid break away and change into Gas. Condensation – is the change of water from its gaseous form (water vapor) into liquid water. Melting – the process when solid like ice changes to liquid (water). Freezing – the process in which a liquid is changed to a solid. Sublimation – the process in which solid changes to gas with no intermediate liquid stage. Desposition – is the phase transition in which gas transformations into solid without passing through the Liquid phase. Vapor – the molecules that escaped from the liquid and go into the gaseous phase. 2/3 The Subatomic Particles Atoms are composed of three particles: 1. Neutrons – does not carry any charges or neutral. 2. Electrons – carries the negative charge (1-). 3. Protons – carries a positive charge (1+). Subatomic Particles – these components of the atom are collectively referred to. Nucleus – contains protons and neutrons. Outer Region – holds the electrons. Atoms – are electrical in nature. - They contain particles with positive and negative charges. Nucleons – the protons and neutrons are called. - Tightly packed together, form the nucleus in the center of the atom. Atomic Number – tells the number of protons in one atom of an element. Mass Number – is the sum of the total number of protons and neutrons in the nucleus of the atom. Isotopes – which are atoms of the same element having the same atomic number but different mass Numbers. Ions – are atoms with extra electrons or missing electrons. Johann Debereiner - 1817 - a German chemist who formed the group of threes or “triads” of elements with similar properties like the triad of calcium, barium and strontium. John Newlands - 1863 - an English chemist proposed the Law of Octaves. Lothar Meyer and Dmitri Mendeleev - 1869 - both came up with periodic tables that showed how elements should be grouped. Henry Moseley - 1913 - a functional relationship that allowed him to use spectral lines to determine the number of protons, and therefore, the atomic number of the elements. Period – single horizontal row in the periodic table. Group or family – each vertical column. Metalloid group – separates the metals from non-metals. Metalloid – is an element that shares some properties with metals and some with non- metals. 3/3 Alkali Metals · Li, Na, K, Rb, Cs, and Fr Alkaline Earth Metals · Be, Mg, Ca, Sr, Ba, and Ra Halogens · F, Cl, Br, I, and At Noble Gases · He, Ne, Ar, Kr, Xe, and Rn Periodic Law – states that when the elements are arranged in order of increasing atomic number, their physical and chemical properties vary periodically. Periodic trends – are specific patterns present in the periodic table that illustrate different aspects of a certain element. Atomic Radius – is an indication of the size of an atom. Ionization energy (IE) – is the amount of energy required to remove the outer electron from an isolated atom. Electronegativity – refers to the electron attracting ability of an atom. Electron Affinity – of an atom is the tendency for that particle to gain an electron. Metallic character – decreases as you move across a period in the periodic table from left to right.