Trends in the Periodic Table
... Name: _________________________________ Period: ____ Date: ___ / ___ / ___ ...
... Name: _________________________________ Period: ____ Date: ___ / ___ / ___ ...
Erin Connors 12/14/10 Chemistry Mrs. Galfunt Atomic Structure
... 8. The atomic 3 is the # of _______ 9. The atomic # is _______ to each element 10. The mass # is the # of ____________ 11. ______________ is the general name for the 2 particles found in the nucleus (_______ & _______) 12. The mass # is written to the ______________ corner of an element’s __________ ...
... 8. The atomic 3 is the # of _______ 9. The atomic # is _______ to each element 10. The mass # is the # of ____________ 11. ______________ is the general name for the 2 particles found in the nucleus (_______ & _______) 12. The mass # is written to the ______________ corner of an element’s __________ ...
Name: _key Date: ______ Period: Unit 3 – Atomic Structure Review
... 2. What was Dalton’s atomic model called? Billard Ball Model 3. Who’s model first introduced the concept of energy levels? Bohr 4. What were the major problems of Dalton’s atomic theory? He was wrong about his first two postulates. 5. Whose model was nicked name the plum pudding model? Thomson 6. Wh ...
... 2. What was Dalton’s atomic model called? Billard Ball Model 3. Who’s model first introduced the concept of energy levels? Bohr 4. What were the major problems of Dalton’s atomic theory? He was wrong about his first two postulates. 5. Whose model was nicked name the plum pudding model? Thomson 6. Wh ...
chapter 2 - WorkNotes
... o The results were astounding [poor Geiger and Marsden first suffered Rutherford’s wrath and were told to try again—this couldn’t be!]. Most of the particles did pass straight through, BUT many were deflected at LARGE angles and some even REFLECTED! Rutherford stated that was like “shooting a ...
... o The results were astounding [poor Geiger and Marsden first suffered Rutherford’s wrath and were told to try again—this couldn’t be!]. Most of the particles did pass straight through, BUT many were deflected at LARGE angles and some even REFLECTED! Rutherford stated that was like “shooting a ...
Atomic Number
... • Use the atomic number given to find the element. • Write the element symbol on the blanks (1st letter of the symbol is capitalized, 2nd (if present) is lower case. • Then write the full name of each element. • Periodic tables can be found in your agenda book or in the textbook inside covers. ...
... • Use the atomic number given to find the element. • Write the element symbol on the blanks (1st letter of the symbol is capitalized, 2nd (if present) is lower case. • Then write the full name of each element. • Periodic tables can be found in your agenda book or in the textbook inside covers. ...
chem 4 outline for exam 1
... (f) an element and a compound Isotopes (Ch. 5, p. 124-126) Explain how we can have 114 known elements, but about 1,000 different kinds of atoms. What is an isotope? Know the meaning of atomic mass. Calculate the atomic mass from percent abundances of the naturally occurring isotopes of an element. I ...
... (f) an element and a compound Isotopes (Ch. 5, p. 124-126) Explain how we can have 114 known elements, but about 1,000 different kinds of atoms. What is an isotope? Know the meaning of atomic mass. Calculate the atomic mass from percent abundances of the naturally occurring isotopes of an element. I ...
CHEM Notes Unit 4 History of atomic theory Monday Oct 7 Greek
... All matter is made of tiny invisible indivisible particles called ATOMS. (definition of element – Boyle) All atoms of the same element are identical and different from atoms of every other element. (definition of element – Boyle; idea of atomic weight – Dalton) Atoms combine in simple whole-nu ...
... All matter is made of tiny invisible indivisible particles called ATOMS. (definition of element – Boyle) All atoms of the same element are identical and different from atoms of every other element. (definition of element – Boyle; idea of atomic weight – Dalton) Atoms combine in simple whole-nu ...
study guide - atomic srtucture/_classification of matter
... idea that all things were made of particles too small to see. He was laughed at. In the 1800’s John Dalton proposed the idea of the “Atomic Theory”. He had 5 theories, 3 of which are still believed today. They are: 1. All matter is composed of extremely small particles too small to see 2. In reactio ...
... idea that all things were made of particles too small to see. He was laughed at. In the 1800’s John Dalton proposed the idea of the “Atomic Theory”. He had 5 theories, 3 of which are still believed today. They are: 1. All matter is composed of extremely small particles too small to see 2. In reactio ...
Matter
... A few elements, such as silicon, have some of the properties of metals and some of the properties of nonmetals. Since they are not clearly one or the other, they are called metalloids, or semimetals. They are used in making semiconductors – materials which can conduct some electricity better than an ...
... A few elements, such as silicon, have some of the properties of metals and some of the properties of nonmetals. Since they are not clearly one or the other, they are called metalloids, or semimetals. They are used in making semiconductors – materials which can conduct some electricity better than an ...
Matter Unit - OG
... 1.) Are made up of only one type of atom. 2) Cannot be broken down into any simpler substances by normal physical or chemical means. 3) Periodic Table of Elements *Familiarize yourself w/ it *Know what those numbers mean! ...
... 1.) Are made up of only one type of atom. 2) Cannot be broken down into any simpler substances by normal physical or chemical means. 3) Periodic Table of Elements *Familiarize yourself w/ it *Know what those numbers mean! ...
Chapter 4
... Every atom has between one and eight valence electrons A valence electron is an electron in the outermost energy level of an atom. They determine an atom’s chemical properties and its ability to form bonds. ...
... Every atom has between one and eight valence electrons A valence electron is an electron in the outermost energy level of an atom. They determine an atom’s chemical properties and its ability to form bonds. ...
Chapter 2 Atoms, Molecules, and Ions
... diagonal staircase line that runs from boron (B) to astatine (At). • Hydrogen, though a nonmetal, is on the left side of the periodic table. • The state of matter at which nonmetals are at room temperature, vary from element to element. ...
... diagonal staircase line that runs from boron (B) to astatine (At). • Hydrogen, though a nonmetal, is on the left side of the periodic table. • The state of matter at which nonmetals are at room temperature, vary from element to element. ...
Goal 5 – Structure and Properties of Matter
... within the nucleus are overcome by the binding force that holds it together. The atomic number of an element is the same as the number of protons and electrons within a neutral atom of that element. Matter is anything that takes up space and has mass. All matter has both physical and chemical proper ...
... within the nucleus are overcome by the binding force that holds it together. The atomic number of an element is the same as the number of protons and electrons within a neutral atom of that element. Matter is anything that takes up space and has mass. All matter has both physical and chemical proper ...
Study Island
... today are the same atoms that were present when the Earth first formed. 3. -4. The atoms of each element differ from those of all other elements in the number of protons. If Ryan found out how many protons the element had, he would be able to identify the element. 5. The elements on the periodic tab ...
... today are the same atoms that were present when the Earth first formed. 3. -4. The atoms of each element differ from those of all other elements in the number of protons. If Ryan found out how many protons the element had, he would be able to identify the element. 5. The elements on the periodic tab ...
Part A: Multiple Choice. Circle the letter
... 6. Most non-metals are located in the periodic table a) on the right hand side b) as the first twenty elements c) in the center d) on the left hand side e) scattered throughout the table 7. In general, which of the following properties does NOT increase across a row from left to right? a) atomic num ...
... 6. Most non-metals are located in the periodic table a) on the right hand side b) as the first twenty elements c) in the center d) on the left hand side e) scattered throughout the table 7. In general, which of the following properties does NOT increase across a row from left to right? a) atomic num ...
Unit 2 Notes Atomic Structures
... theory. He believed that different atoms or elements could be distinguished by their weight. While working on your theory you discovered the law of multiple proportions which states that when combining two or more elements to form a chemical compound, the elements are always in the smallest whole nu ...
... theory. He believed that different atoms or elements could be distinguished by their weight. While working on your theory you discovered the law of multiple proportions which states that when combining two or more elements to form a chemical compound, the elements are always in the smallest whole nu ...
Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table
... - The atomic number is typically found _______________________ of each element square - It shows how many ___________ are in one atom of that element. - Atoms have a ____________ charge, therefore the number of __________________ equals the number of __________________ - As you move across the perio ...
... - The atomic number is typically found _______________________ of each element square - It shows how many ___________ are in one atom of that element. - Atoms have a ____________ charge, therefore the number of __________________ equals the number of __________________ - As you move across the perio ...
Chapter 4
... • We know atoms are composed of three main pieces - protons, neutrons and electrons • The nucleus contains protons and neutrons • The nucleus is only about 10-13 cm in diameter • The electrons move outside the nucleus with an average distance of about 10-8 cm – therefore the radius of the atom is ab ...
... • We know atoms are composed of three main pieces - protons, neutrons and electrons • The nucleus contains protons and neutrons • The nucleus is only about 10-13 cm in diameter • The electrons move outside the nucleus with an average distance of about 10-8 cm – therefore the radius of the atom is ab ...
Name________________________________________
... • Their mass is so small that it is usually considered ___________. • It takes more than 1,800 electrons to equal the mass of one proton. • However electrons occupy most of an atoms ______________. Some things to remember: • In an atom, the number of protons equals the number of electrons. As a resu ...
... • Their mass is so small that it is usually considered ___________. • It takes more than 1,800 electrons to equal the mass of one proton. • However electrons occupy most of an atoms ______________. Some things to remember: • In an atom, the number of protons equals the number of electrons. As a resu ...
File - Biochemistry
... atoms are the smallest particles and each substance had its own type of atom - wood atoms, air atoms, water atoms Dalton: 1. all matter is made of tiny particles called atoms 2. atoms can’t be broken down further 3. atoms of different elements differ 4. atoms of the same element are identical 5. ato ...
... atoms are the smallest particles and each substance had its own type of atom - wood atoms, air atoms, water atoms Dalton: 1. all matter is made of tiny particles called atoms 2. atoms can’t be broken down further 3. atoms of different elements differ 4. atoms of the same element are identical 5. ato ...
Chemical element
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A chemical element (or element) is a chemical substance consisting of atoms having the same number of protons in their atomic nuclei (i.e. the same atomic number, Z). There are 118 elements that have been identified, of which the first 94 occur naturally on Earth with the remaining 24 being synthetic elements. There are 80 elements that have at least one stable isotope and 38 that have exclusively radioactive isotopes, which decay over time into other elements. Iron is the most abundant element (by mass) making up the Earth, while oxygen is the most common element in the crust of the earth.Chemical elements constitute approximately 15% of the matter in the universe: the remainder is dark matter, the composition of it is unknown, but it is not composed of chemical elements.The two lightest elements, hydrogen and helium were mostly formed in the Big Bang and are the most common elements in the universe. The next three elements (lithium, beryllium and boron) were formed mostly by cosmic ray spallation, and are thus more rare than those that follow. Formation of elements with from six to twenty six protons occurred and continues to occur in main sequence stars via stellar nucleosynthesis. The high abundance of oxygen, silicon, and iron on Earth reflects their common production in such stars. Elements with greater than twenty six protons are formed by supernova nucleosynthesis in supernovae, which, when they explode, blast these elements far into space as planetary nebulae, where they may become incorporated into planets when they are formed.When different elements are chemically combined, with the atoms held together by chemical bonds, they form chemical compounds. Only a minority of elements are found uncombined as relatively pure minerals. Among the more common of such ""native elements"" are copper, silver, gold, carbon (as coal, graphite, or diamonds), and sulfur. All but a few of the most inert elements, such as noble gases and noble metals, are usually found on Earth in chemically combined form, as chemical compounds. While about 32 of the chemical elements occur on Earth in native uncombined forms, most of these occur as mixtures. For example, atmospheric air is primarily a mixture of nitrogen, oxygen, and argon, and native solid elements occur in alloys, such as that of iron and nickel.The history of the discovery and use of the elements began with primitive human societies that found native elements like carbon, sulfur, copper and gold. Later civilizations extracted elemental copper, tin, lead and iron from their ores by smelting, using charcoal. Alchemists and chemists subsequently identified many more, with almost all of the naturally-occurring elements becoming known by 1900. The properties of the chemical elements are summarized on the periodic table, which organizes the elements by increasing atomic number into rows (""periods"") in which the columns (""groups"") share recurring (""periodic"") physical and chemical properties. Save for unstable radioactive elements with short half-lives, all of the elements are available industrially, most of them in high degrees of purity.