Chemistry Name_______________________ Chapter 4
... Democritus believed these atoms could move through empty space. Aristotle did not believe in empty space ...
... Democritus believed these atoms could move through empty space. Aristotle did not believe in empty space ...
chemical periodicity
... – 1. AR increases going down in a group – 2. AR decreases going left to right in a period ...
... – 1. AR increases going down in a group – 2. AR decreases going left to right in a period ...
Chemistry Module 1- Basic Revision Notes 1.1a Atomic Structure 1.1
... By looking at the above table, you can see that the last number in the electronic structure, corresponds with the group number e.g. 2.1 = group I 2.5 = group V Also the electronic structure gives the period number e.g. 2.1 = period 2 2.8.1 = period 3 Plus the total number of electrons gives th ...
... By looking at the above table, you can see that the last number in the electronic structure, corresponds with the group number e.g. 2.1 = group I 2.5 = group V Also the electronic structure gives the period number e.g. 2.1 = period 2 2.8.1 = period 3 Plus the total number of electrons gives th ...
Periodic Law
... These elements look different, but have similar chemical properties: they react easily with metals Unfortunately, all the known elements could not be grouped into triads. ...
... These elements look different, but have similar chemical properties: they react easily with metals Unfortunately, all the known elements could not be grouped into triads. ...
CHEM 481. Chapter 1. Atomic stucture and periodic table. Answers
... All the magnitudes increase from left to right across the period, since each trend reflects the increasing Z* as electrons are being added to orbitals of the same shell. For IP, this reflects the difficulty of removing an electron. For EG enthalpy, this reflects energy released when an additional el ...
... All the magnitudes increase from left to right across the period, since each trend reflects the increasing Z* as electrons are being added to orbitals of the same shell. For IP, this reflects the difficulty of removing an electron. For EG enthalpy, this reflects energy released when an additional el ...
Radioactive Isotopes and Nuclear Equations
... Atoms are composed of three subatomic particles: protons, neutrons and electrons. Protons and neutrons are found in the nucleus of an atom. The total number of protons and neutrons determines an atom’s mass. The number of protons defines the element. Some nuclei are unstable, so they decompose (or " ...
... Atoms are composed of three subatomic particles: protons, neutrons and electrons. Protons and neutrons are found in the nucleus of an atom. The total number of protons and neutrons determines an atom’s mass. The number of protons defines the element. Some nuclei are unstable, so they decompose (or " ...
Atomic Structure - Learn District 196
... • If you change the number of protons, you change the type of atom itself. • If you change the number of electrons, you change the atom to an ion (charged particle). • If you change the number of neutrons, you change the isotope of that element. ...
... • If you change the number of protons, you change the type of atom itself. • If you change the number of electrons, you change the atom to an ion (charged particle). • If you change the number of neutrons, you change the isotope of that element. ...
4.9 Bohr`s Theory of the Atom
... • Time for a new theory! In order for a new theory to emerge, more data was necessary. • Einstein found that data. He examined the light given off by pure elemental gas viewed through a prism. What he found was surprising. Instead of a steady rainbow he found that there were bright ...
... • Time for a new theory! In order for a new theory to emerge, more data was necessary. • Einstein found that data. He examined the light given off by pure elemental gas viewed through a prism. What he found was surprising. Instead of a steady rainbow he found that there were bright ...
Periodicity - Walton High
... 1914 that elements’ properties more closely followed their atomic number • Modern Periodic Table based on this discovery ...
... 1914 that elements’ properties more closely followed their atomic number • Modern Periodic Table based on this discovery ...
Fall 2015 Review-2
... ____ 14. The atomic mass of an element is the ____. a. total number of subatomic particles in its nucleus b. weighted average of the masses of the isotopes of the element c. total mass of the isotopes of the element d. average of the mass number and the atomic number for the element ____ 15. If thre ...
... ____ 14. The atomic mass of an element is the ____. a. total number of subatomic particles in its nucleus b. weighted average of the masses of the isotopes of the element c. total mass of the isotopes of the element d. average of the mass number and the atomic number for the element ____ 15. If thre ...
Atomic Structure
... • If you change the number of protons, you change the type of atom itself. • If you change the number of electrons, you change the atom to an ion (charged particle). • If you change the number of neutrons, you change the isotope of that element. ...
... • If you change the number of protons, you change the type of atom itself. • If you change the number of electrons, you change the atom to an ion (charged particle). • If you change the number of neutrons, you change the isotope of that element. ...
Periodicity - Walton High
... 1914 that elements’ properties more closely followed their atomic number • Modern Periodic Table based on this discovery ...
... 1914 that elements’ properties more closely followed their atomic number • Modern Periodic Table based on this discovery ...
Periodic Table and Electrons
... Metalloids have properties of metals and nonmetals. They are located between metals and nonmetals on the periodic table. Some are used in semiconductors. Periods and groups are named by numbering columns and rows. Horizontal rows called periods have predictable properties based on an increasing numb ...
... Metalloids have properties of metals and nonmetals. They are located between metals and nonmetals on the periodic table. Some are used in semiconductors. Periods and groups are named by numbering columns and rows. Horizontal rows called periods have predictable properties based on an increasing numb ...
History of the Atom
... o This nucleus is made up of particles called protons, which have a positive ...
... o This nucleus is made up of particles called protons, which have a positive ...
6-1-Periodic Law
... It was found that if Mendeleev's table was ordered by atomic number instead of atomic mass the inconsistencies in the table were eliminated. This is the blueprint for the modern periodic table. ...
... It was found that if Mendeleev's table was ordered by atomic number instead of atomic mass the inconsistencies in the table were eliminated. This is the blueprint for the modern periodic table. ...
Atomic Theory
... That’s right. Niels Bohr developed the model that you are talking about in 1920. He observed that when energy was added to an atom, electrons could use that energy to move farther away from the nucleus. However, they did not just move anywhere. They were much more likely to be in some places than ot ...
... That’s right. Niels Bohr developed the model that you are talking about in 1920. He observed that when energy was added to an atom, electrons could use that energy to move farther away from the nucleus. However, they did not just move anywhere. They were much more likely to be in some places than ot ...
Pre-AP Review Unit 2
... 15. All atoms are neutral because the number of __________________ always equals the number of __________________ in every atom. Fill in the chart with a charge and mass: ...
... 15. All atoms are neutral because the number of __________________ always equals the number of __________________ in every atom. Fill in the chart with a charge and mass: ...
Atoms, Molecules, and Ions
... Both atoms become charged and are called ions Anion: atom gaining the electron is negatively charged Cation: atom losing the electron is positively charged ...
... Both atoms become charged and are called ions Anion: atom gaining the electron is negatively charged Cation: atom losing the electron is positively charged ...
Chapter 17 Notes
... • In the _____________, the elements are arranged by increasing atomic number and by changes in physical and chemical properties. • On Mendeleev's table, the atomic mass gradually increased from left to right. If you look at the modern periodic table, you will see several examples, such as cobalt an ...
... • In the _____________, the elements are arranged by increasing atomic number and by changes in physical and chemical properties. • On Mendeleev's table, the atomic mass gradually increased from left to right. If you look at the modern periodic table, you will see several examples, such as cobalt an ...
Topic 7. 1 Atomic Structure
... When nuclei of the same element have different numbers of neutrons. Carbon has 6 isotopes: Carbon-11, Carbon-12, Carbon-13, Carbon-14, Carbon-15, Carbon-16. All have 6 protons but each has different number of neutrons. The different isotopes don’t exist in nature in equal amounts. Carbon: ...
... When nuclei of the same element have different numbers of neutrons. Carbon has 6 isotopes: Carbon-11, Carbon-12, Carbon-13, Carbon-14, Carbon-15, Carbon-16. All have 6 protons but each has different number of neutrons. The different isotopes don’t exist in nature in equal amounts. Carbon: ...
Atomic Structure Notes
... charged nucleus was surrounded by a great deal of "empty space" through which the electrons moved. • In 1911, Robert Millikan conducted his "oil-drop" experiment which allowed him to measure the charge on an electron. Combining his results with those of Thomson, Millikan found the mass of the electr ...
... charged nucleus was surrounded by a great deal of "empty space" through which the electrons moved. • In 1911, Robert Millikan conducted his "oil-drop" experiment which allowed him to measure the charge on an electron. Combining his results with those of Thomson, Millikan found the mass of the electr ...
PHYSICAL SCIENCE -- CHAPTER 10 READING GUIDE
... 13. Oxygen occurs in nature as a mix of two isotopes: 16O and 17O. Look at the periodic table -- the average atomic mass of oxygen is __________. Which isotope of oxygen do you think is: less than 1% of naturally occuring oxygen? ______________ more than 99% of naturally occuring oxygen? ___________ ...
... 13. Oxygen occurs in nature as a mix of two isotopes: 16O and 17O. Look at the periodic table -- the average atomic mass of oxygen is __________. Which isotope of oxygen do you think is: less than 1% of naturally occuring oxygen? ______________ more than 99% of naturally occuring oxygen? ___________ ...
Chapter 4 Structure of Atoms Isotopes and Ions KEY
... 1. List the charge and location of protons, neutrons and electrons in an atom. protons positive one, Nucleus Elecrons- negative one, -1, in electron cloud neutrons no charge, nucleus 2. List the relative mass of protons, neutrons and electrons in an atom. Relative mass means the mass compared to the ...
... 1. List the charge and location of protons, neutrons and electrons in an atom. protons positive one, Nucleus Elecrons- negative one, -1, in electron cloud neutrons no charge, nucleus 2. List the relative mass of protons, neutrons and electrons in an atom. Relative mass means the mass compared to the ...