![Unit 5: Atoms and the Periodic Table](http://s1.studyres.com/store/data/008517085_1-a0726c5f80c6aac44a80684e17b71a90-300x300.png)
1st semester exam review
... • John Newlands – Noticed when elements were arranged by increasing atomic mass their properties repeated every 8th element • Pattern is periodic (repeats in a specific manner) ...
... • John Newlands – Noticed when elements were arranged by increasing atomic mass their properties repeated every 8th element • Pattern is periodic (repeats in a specific manner) ...
Chapter One Powerpoint - Geneva Area City Schools
... Introduction to the Periodic Table • All known elements are organized into a chart known as the periodic table • The vertical columns of the periodic table are called groups, or families. • Each group contains elements with similar chemical properties. • The horizontal rows of elements in the perio ...
... Introduction to the Periodic Table • All known elements are organized into a chart known as the periodic table • The vertical columns of the periodic table are called groups, or families. • Each group contains elements with similar chemical properties. • The horizontal rows of elements in the perio ...
Name: : ______ Chemistry—Matter, Atoms, and More Visit the
... _________________. Matter is anything that has a _________________. As of ___________ scientists have identified ___________________ states of matter. 12. You should know about ______________, _______________, _______________, and plasmas, and a new one called ________________-__________________ __ ...
... _________________. Matter is anything that has a _________________. As of ___________ scientists have identified ___________________ states of matter. 12. You should know about ______________, _______________, _______________, and plasmas, and a new one called ________________-__________________ __ ...
final exam practice test - Clayton State University
... b. The presence of lone (unshared) pairs of electrons affect the dipole moment of a molecule. c. Generally, as electronegativity differences increases in diatomic molecules, the dipole moments increase. d. The dipole moment equals the product of charge and distance of separation of the charges. e. B ...
... b. The presence of lone (unshared) pairs of electrons affect the dipole moment of a molecule. c. Generally, as electronegativity differences increases in diatomic molecules, the dipole moments increase. d. The dipole moment equals the product of charge and distance of separation of the charges. e. B ...
Name - Madison County Schools
... D. What do elements that belong to the same group have in common? They have the same number of valence electrons; similar chemical properties E. What is the “octet rule”? Atoms are most stable if they have filled or empty outer shell of electrons Filled shell contains 8 electrons (octet) Except for ...
... D. What do elements that belong to the same group have in common? They have the same number of valence electrons; similar chemical properties E. What is the “octet rule”? Atoms are most stable if they have filled or empty outer shell of electrons Filled shell contains 8 electrons (octet) Except for ...
Avg. Atomic Mass - Greer Middle College
... The nucleus is tiny compared to the atom as a whole. Rutherford reasoned that all of an atom’s positively charged particles were contained in the nucleus. The negatively charged particles were scattered outside the nucleus around the atom’s edge. 1932 – James Chadwick confirmed the existence o ...
... The nucleus is tiny compared to the atom as a whole. Rutherford reasoned that all of an atom’s positively charged particles were contained in the nucleus. The negatively charged particles were scattered outside the nucleus around the atom’s edge. 1932 – James Chadwick confirmed the existence o ...
Name Period _____ Table _____ Vocabulary Log: ATOMS
... The particle of an atom with no charge. Most atoms have the same number of protons and neutrons, but some isotopes of an element have a different number of neutrons. (ALL atoms of an element will have the same number of protons.) ...
... The particle of an atom with no charge. Most atoms have the same number of protons and neutrons, but some isotopes of an element have a different number of neutrons. (ALL atoms of an element will have the same number of protons.) ...
Structure of the Atom JJ Thomson- discovered the electron in late
... With the discovery of the neutron, it was also discovered that atoms could contain varied numbers of neutrons. Dalton’s atomic theory has to be modified to reflect this discovery. Dalton’s Atomic Theory – 1808 #2 All atoms of a given element are identical. #2 is modified to: All atoms of a given ele ...
... With the discovery of the neutron, it was also discovered that atoms could contain varied numbers of neutrons. Dalton’s atomic theory has to be modified to reflect this discovery. Dalton’s Atomic Theory – 1808 #2 All atoms of a given element are identical. #2 is modified to: All atoms of a given ele ...
Early Atomic Theory - Columbia University
... a calcium ion It is 58.69 / 10.81 = 5.29 times as heavy as a boron ion Element ...
... a calcium ion It is 58.69 / 10.81 = 5.29 times as heavy as a boron ion Element ...
Unit 2 Notes unit_2_atomic-nuclear-electronic
... lowest energy levels are close to the nucleus. The farther from the nucleus corresponds to higher energy levels. Electrons tend to occupy the lowest energy levels available. 3)Light is emitted when an electron jumps from a higher orbit to a lower orbit. Light is absorbed when it jumps from a lower t ...
... lowest energy levels are close to the nucleus. The farther from the nucleus corresponds to higher energy levels. Electrons tend to occupy the lowest energy levels available. 3)Light is emitted when an electron jumps from a higher orbit to a lower orbit. Light is absorbed when it jumps from a lower t ...
AS II Rutherford Model
... even though the 3 of subatomic particles are whole-number multiples, the atomic masses are not; (xs mass as you go from lower to higher atoms converted to energy) ...
... even though the 3 of subatomic particles are whole-number multiples, the atomic masses are not; (xs mass as you go from lower to higher atoms converted to energy) ...
Bohr Atomic Model - Flinn Scientific
... electrons. According to the Bohr model, the electrons were restricted to certain specific orbits around the nucleus of the atom. These orbits differed in their distance from the nucleus and in their energy levels. Electrons that are closer to the nucleus are lower in energy than electrons that are f ...
... electrons. According to the Bohr model, the electrons were restricted to certain specific orbits around the nucleus of the atom. These orbits differed in their distance from the nucleus and in their energy levels. Electrons that are closer to the nucleus are lower in energy than electrons that are f ...
History of the Atom
... Proved that an atom can be divided into smaller parts While experimenting with cathoderay tubes, discovered “corpuscles”, which were later called electrons Stated that the atom is neutral In 1897, proposed the Plum Pudding Model which states that atoms mostly consist of positively charged ma ...
... Proved that an atom can be divided into smaller parts While experimenting with cathoderay tubes, discovered “corpuscles”, which were later called electrons Stated that the atom is neutral In 1897, proposed the Plum Pudding Model which states that atoms mostly consist of positively charged ma ...
Academic Chemistry
... 14. Which of the following statements explains why chemists do not count atoms and molecules directly? A. Atoms and molecules are extremely small B. All of the relationships in a chemical reaction can be expressed as mass ratios C. Matter is neither created nor destroyed in a chemical reaction D. Re ...
... 14. Which of the following statements explains why chemists do not count atoms and molecules directly? A. Atoms and molecules are extremely small B. All of the relationships in a chemical reaction can be expressed as mass ratios C. Matter is neither created nor destroyed in a chemical reaction D. Re ...
Unit 2 Atomic Structure and Matter
... Models are not completely accurate. They represent something that is not easily seen or understood ...
... Models are not completely accurate. They represent something that is not easily seen or understood ...
atomic-models
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
... • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. ...
atomic mass - Cloudfront.net
... because of its protons. • In a neutral atom the proton # = electron # • B = Boron = __p+, __e• Cl = Chlorine = ____p+, ____e- ...
... because of its protons. • In a neutral atom the proton # = electron # • B = Boron = __p+, __e• Cl = Chlorine = ____p+, ____e- ...
File
... 6. The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following? A. Na has a greater density at standard conditions than Ne. B. Na has a lo ...
... 6. The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following? A. Na has a greater density at standard conditions than Ne. B. Na has a lo ...
Atomic Theory
... __________ _________, similarities in their properties occur in a regular pattern. a) Atomic mass b) Atomic number c) Atomic radius ...
... __________ _________, similarities in their properties occur in a regular pattern. a) Atomic mass b) Atomic number c) Atomic radius ...
Chemistry Midterm Review Study Guide 2012
... 4. a. Which has the larger radius, Al or In? In b. Which has the larger radius, Se or Ca? Ca c. Which has a larger radius, Ca or Ca+2 Ca (would get smaller if lost 2 e-) d. Which has greater ionization energies as a class, metals or nonmetals? nonmetals e. Which has the greater ionization energy, As ...
... 4. a. Which has the larger radius, Al or In? In b. Which has the larger radius, Se or Ca? Ca c. Which has a larger radius, Ca or Ca+2 Ca (would get smaller if lost 2 e-) d. Which has greater ionization energies as a class, metals or nonmetals? nonmetals e. Which has the greater ionization energy, As ...
Periodic table
The periodic table is a tabular arrangement of the chemical elements, ordered by their atomic number (number of protons in the nucleus), electron configurations, and recurring chemical properties. The table also shows four rectangular blocks: s-, p- d- and f-block. In general, within one row (period) the elements are metals on the lefthand side, and non-metals on the righthand side.The rows of the table are called periods; the columns are called groups. Six groups (columns) have names as well as numbers: for example, group 17 elements are the halogens; and group 18, the noble gases. The periodic table can be used to derive relationships between the properties of the elements, and predict the properties of new elements yet to be discovered or synthesized. The periodic table provides a useful framework for analyzing chemical behavior, and is widely used in chemistry and other sciences.Although precursors exist, Dmitri Mendeleev is generally credited with the publication, in 1869, of the first widely recognized periodic table. He developed his table to illustrate periodic trends in the properties of the then-known elements. Mendeleev also predicted some properties of then-unknown elements that would be expected to fill gaps in this table. Most of his predictions were proved correct when the elements in question were subsequently discovered. Mendeleev's periodic table has since been expanded and refined with the discovery or synthesis of further new elements and the development of new theoretical models to explain chemical behavior.All elements from atomic numbers 1 (hydrogen) to 118 (ununoctium) have been discovered or reportedly synthesized, with elements 113, 115, 117, and 118 having yet to be confirmed. The first 94 elements exist naturally, although some are found only in trace amounts and were synthesized in laboratories before being found in nature. Elements with atomic numbers from 95 to 118 have only been synthesized in laboratories. It has been shown that einsteinium and fermium once occurred in nature but currently do not. Synthesis of elements having higher atomic numbers is being pursued. Numerous synthetic radionuclides of naturally occurring elements have also been produced in laboratories.