Atoms are made of protons, electrons, and neutrons. Protons and neutrons are located inside the nucleus that is at the center of an atom. Electrons occupy orbitals, which are located outside the nucleus. In this module, you will study the structure of atoms.
Atoms are the building blocks of matter. Every living and non-living thing is made of atoms. Those same atoms make up elements. For example, gold is an element and is made of gold atoms.
Atoms are the basic building blocks of matter that make up everyday objects. A desk, the air, even you are made up of atoms!
There are 90 naturally occurring kinds of atoms. Scientists in labs have been able to make about 25 more.
Protons- carry a positive charge -1 amu= heavy
In 1968 new particles were discovered inside the proton called quarks.
There are 3 quarks in each proton and gluons hold them together
Neutrons carry no charge- discovered in 1932- also have quarks and gluons
Protons and neutrons join together to build the nucleus- the central part of the atom
Electrons carry a negative charge and circle the nucleus- electrons are extremely small and very light
Electrons are easy to strip off an atom and use for electrical power
Electrons can tell about the inside of an atom atomic number = number of protons isotopes mass number = number of protons+ neutrons s=1 p=3 d=5 f=7 each orbital can hold 2 electrons
2n^2 can be used to calculate the max number of electrons in the nth level
Orbitals are regions where electrons are likely to be found
The periodic table is an organized list of all the elements known to us. It contains key information about the elements such as atomic number, atomic mass, symbols, names of the elements, relative sizes of atoms, reactivity and more. It is an essential chart that chemists cannot do without. In this module you will learn the organization of the periodic table.
Columns-= groups
Rows=periods
The first column of the periodic table is the group of elements known as the Group 1 or alkali metals. This group includes lithium, sodium, potassium, rubidium, cesium, and francium. By definition, a metal is an element that loses one or more electrons to create a positively charged ion known as a cation (pronounced "cat"- "ion")
The second column of elements from the left of the periodic table is known as the Group 2 or alkaline earth metals. It consists of beryllium, magnesium, calcium, strontium, barium, and radium.
The group of elements at the far right of the table (Group 18) is known commonly as the noble gases. They are generally chemically inert. This means that they do not react with other elements because they already have the desired eight total s and p electrons in their outermost (highest) energy level. The elements in this group are helium, neon, argon, krypton, xenon, and radon. They are monatomic gases.
Group 17 is a family of elements known as the halogens. The word "halogen" means "salt-former." The halogens form salts when they react with a metal. Halogens exist in a variety of states at room temperature. Fluorine and chlorine are gases, bromine is a liquid, and iodine and astatine are solids.
Group 16 is the oxygen family. It consists of the elements oxygen, sulfur, selenium, tellurium, and polonium.
The Group 15 elements are generally known as the nitrogen family. All of the elements of this family have five electrons in their outermost energy level. This group is divided into nonmetals, semimetals, and metals by characteristic. The top two elements, nitrogen and phosphorus, are very definitely nonmetals, forming -3 charge anions. Nitrogen is a diatomic gas and phosphorus is a solid. The elements arsenic, antimony, and bismuth all have some characteristics of semimetals such as brittleness as a free element.
Group 14 is the carbon family. The five members are carbon, silicon, germanium, tin, and lead.
The last of the p block families we will be looking at is the boron family -- Group 13. This
Chemistry Overview: 4 major elements (C, H, O, N) pH Water’s role in the body A lot of terminology! An atom- smallest unit of Stable matter Ex. Carbon, Hydrogen, Oxygen, Nitrogen Subatomic Particles Proton: Positive charge, 1 mass unit Neutron: Neutral charge, 1 mass unit Electron: Negative charge, low mass Ions If protons are not equal to electrons the atom is now known as an ion Cation = (+) Anion = (-) Valence Shell vs. Core Electrons Valence (outer) electron shells “Want” to be filled More stable…
Chemistry Master Notes Covalent Bonding In a covalent bond electrons are shared between two atoms. Hydrogen is diatomic, energy is released when bonds are formed making H2 more stable. Molecules with a full outer shell become noble gas forms, very unreactive. Ionic Bonding Electrically charged ions are called Ions Positive = cation Negative = anion Metallic Bonding In the example of Na, the outer electron of each atom becomes ‘delocalised’ and free to…
Sodium hydroxide NaOH Sodium oxide Na2O Barium hydroxide BaOH2 Calcium oxide CaO Neutralisation reaction acid + base -> salt + water e.g 2HCl + CaO -> CaCl2 + H2O Syllabus Notes 9.3.2.2.4 Identify factors which can affect the equilibrium in a reversible reaction 1. Temperature 2. Concentration 3. Pressure/ Volume Note: catalysts don’t alter the position of a system already in equilibrium. If system is not at equilibrium, catalyst will only help it reach equilibrium faster. It lowers the activation…
Chemistry H Ch.7-8 Test Study Guide Ion formation, gain/lose electrons: - Ions are formed when an atom gains or loses electrons and get charged. - If an atom gains electrons, an atom gets negatively charged (Anion). - Similarly if an atom looses electrons, the atom becomes positively charged (Cation). Ionic Compounds, properties: - A compound that is composed entirely of ions is called an ionic compound. - Ionic compounds are formed from a metal and a non-metal. - Ionic compounds…
notes 8.1 & 3.5 & pg 85 1-5 8.1 molecular equation for the reaction; it shows the complete formulas of all reactants and products Ions such as these, which do not participate directly in a reaction in solution, are called spectator ions net ionic equation, includes only those components that are directly involved in the reaction a. Molecular equation: NaCl(aq) _ AgN O3 (aq) n AgCl(s) _ NaN O3 (aq) Complete ionic equation: N a_ (aq)…
Chemistry: The branch of science that considers the composition of matter and how this composition changes. Element: A chemical substance with only one type of atom. Atom: Smallest particle of an element that has the properties of that element. Nucleus: The dense core of an atom composed of protons and neutrons. Electron: A small, negatively charged particle that revolves around the nucleus of an atom. Proton: A positively charged particle in an atomic nucleus. Neutron: An electrically neutral…
Chemistry Physical Property: A physical property is one that is displayed without any change in composition Chemical Property: Any characteristic that gives a sample of matter the ability/inability to undergo a change that alters its composition. Examples: Alkali metals react with water; Paper's ability to burn. Physical Change: Change in which the matter's physical appearance is altered, but composition remains unchanged. (Change in state of matter) Chemical Change: Change in which one or more kinds…
Nonpolar Bond- A bond formed by sharing a pair of electrons between two atoms of the same element or atoms with the same electronegativity Nonpolar Molecule- A molecule that has a symmetrical shape and a symmetrical charge distribution, such as F2, CCl4 or CO2 Element- A substance that cannot be decomposed by chemical change All known elements are listed in the Periodic Table. Ionic Bond- A bond resulting from the transfer of an electron from one atom to another An ionic bond is formed by the transfer…
Science- chemistry notes Definitions: Atoms: Tiny particles that make up all matter. Atoms are made up of protons, neutrons and electrons. Protons and neutrons are heavier than electrons and are located at the centre of the atom, the nucleus. The electrons spin around the nucleus in a region of empty space. Neutrons are neutral-no charge. Protons-have a positive charge. Electrons-have a negative charge. Opposite charges attract each other and this is what keeps the electrons…