Subatomic notes - Chemistry R: 4(AE) 5(A,C)
... the radius of the nucleus to be less than 1/10,000 of the atom. – If the nucleus were the size of a marble, the atom would be the size of a football stadium ...
... the radius of the nucleus to be less than 1/10,000 of the atom. – If the nucleus were the size of a marble, the atom would be the size of a football stadium ...
Glencoe Chapter 4 Structure of the Atom for the Wiki
... Based on atomic theory but no experiment evidence at the time • The ratio of the masses of one element that combine with a constant mass of another element can be expressed in small whole numbers. ...
... Based on atomic theory but no experiment evidence at the time • The ratio of the masses of one element that combine with a constant mass of another element can be expressed in small whole numbers. ...
Subatomic Particles Do Now • What is an atom?
... the radius of the nucleus to be less than 1/10,000 of the atom. – If the nucleus were the size of a ________, the atom would be the size of a __________________ ...
... the radius of the nucleus to be less than 1/10,000 of the atom. – If the nucleus were the size of a ________, the atom would be the size of a __________________ ...
Proton Positively charged subatomic (smaller than an atom) particle
... helps hold protons inside the nucleus. ...
... helps hold protons inside the nucleus. ...
Atomic Theory
... __________ _________, similarities in their properties occur in a regular pattern. a) Atomic mass b) Atomic number c) Atomic radius Moseley created the modern periodic table when he determined that elements should be placed in order of increasing atomic number (# of protons). It’s a shame that WWI t ...
... __________ _________, similarities in their properties occur in a regular pattern. a) Atomic mass b) Atomic number c) Atomic radius Moseley created the modern periodic table when he determined that elements should be placed in order of increasing atomic number (# of protons). It’s a shame that WWI t ...
gained (-) or lost (+) an electron
... Remember: Atomic Mass or Mass # is the more massive number on the element ...
... Remember: Atomic Mass or Mass # is the more massive number on the element ...
Unit 4
... ● Atoms are made up of 3 subatomic particles; protons, neutrons, and electrons. ● The history of atomic development shaped the way scientists have constructed the current model of the atom. ...
... ● Atoms are made up of 3 subatomic particles; protons, neutrons, and electrons. ● The history of atomic development shaped the way scientists have constructed the current model of the atom. ...
What do we call a substance with more than one kind of atom
... 40. When using the spectrometer we noticed that depending upon which elemental gas is used to produce the light, different lines of the spectrum will appear. If the predominant band is red, what could you hypothesize about the waves that created these bands with regard to energy and wavelength? 41. ...
... 40. When using the spectrometer we noticed that depending upon which elemental gas is used to produce the light, different lines of the spectrum will appear. If the predominant band is red, what could you hypothesize about the waves that created these bands with regard to energy and wavelength? 41. ...
Chapter 8: Periodic Properties of the Elements
... lower in energy than d orbitals of the previous principal level (4s is lower than 3d) • The energy separations between one set of orbitals and the next become smaller beyond the 4s so the ordering can vary among elements causing variations (exceptions) in the electron configurations of the transitio ...
... lower in energy than d orbitals of the previous principal level (4s is lower than 3d) • The energy separations between one set of orbitals and the next become smaller beyond the 4s so the ordering can vary among elements causing variations (exceptions) in the electron configurations of the transitio ...
atoms
... University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons. ...
... University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons. ...
30.09.2013 1 Chapter 2 Atoms and Molecules Warning!! Chapter
... • The exchange or sharing of electrons results in lower energy for the compound relative to the separate atoms. • Ionic: exchange; cations and anions present • Metallic: sharing by forming a mobile “sea of electrons” • Covalent: sharing between atoms ...
... • The exchange or sharing of electrons results in lower energy for the compound relative to the separate atoms. • Ionic: exchange; cations and anions present • Metallic: sharing by forming a mobile “sea of electrons” • Covalent: sharing between atoms ...
Atomic Structure - Madison County Schools
... • Elements were originally placed in the periodic table based on their repeating properties, which are a result of the number and type of valence electrons. • Properties of an element can be predicted based on its placement in the periodic table. Groups of elements exhibit similar properties with pr ...
... • Elements were originally placed in the periodic table based on their repeating properties, which are a result of the number and type of valence electrons. • Properties of an element can be predicted based on its placement in the periodic table. Groups of elements exhibit similar properties with pr ...
What are elements?
... blocks of all matter. • The periodic table is a list of all of the elements that can build matter. It’s a little like the alphabet of chemistry. • The periodic table tells us several things… ...
... blocks of all matter. • The periodic table is a list of all of the elements that can build matter. It’s a little like the alphabet of chemistry. • The periodic table tells us several things… ...
8th Grade
... 15. Who was the Greek philosopher who lived 2300 years ago, and what did he think? _________________________________________________________________________________________ 16. In 1800 another scientist added to the idea of the Greek guy. Who was this man and what was his idea? ____________________ ...
... 15. Who was the Greek philosopher who lived 2300 years ago, and what did he think? _________________________________________________________________________________________ 16. In 1800 another scientist added to the idea of the Greek guy. Who was this man and what was his idea? ____________________ ...
AP Projectile Motion
... number of protons in a nucleus exactly matches the number of electrons around the nucleus in a neutral atom, number of protons in the nucleus need not match the number of neutrons there all hydrogen nuclei have a single proton but most have no neutrons. small percentage contain one neutron and a sma ...
... number of protons in a nucleus exactly matches the number of electrons around the nucleus in a neutral atom, number of protons in the nucleus need not match the number of neutrons there all hydrogen nuclei have a single proton but most have no neutrons. small percentage contain one neutron and a sma ...
Chapter 16: The Properties of Atoms and the Periodic Table
... The Greeks thought that an atom of fire would look like a very small flame, water like a very small bit of water, and so on All matter consisted of these atoms or mixtures of the atoms • The problem with the Greek idea of the atom is that they could not test to see if it was correct In the early ...
... The Greeks thought that an atom of fire would look like a very small flame, water like a very small bit of water, and so on All matter consisted of these atoms or mixtures of the atoms • The problem with the Greek idea of the atom is that they could not test to see if it was correct In the early ...
Atoms
... NSES B1a. Matter is made of minute particles called atoms, and atoms are composed of even smaller components. These components have measurable properties, such as mass and electrical charge. Each atom has a positively charged nucleus surrounded by negatively charged electrons. The electric force bet ...
... NSES B1a. Matter is made of minute particles called atoms, and atoms are composed of even smaller components. These components have measurable properties, such as mass and electrical charge. Each atom has a positively charged nucleus surrounded by negatively charged electrons. The electric force bet ...
Chapter 5
... Review for exam 2 (Chapters 4 (all), 5 (all), 6 (6.1 to 6.3)) Chapter 4 The periodic table general organization of the table, rows (periods) and columns (groups) main group, transition metals, lanthanides, actinides valence electrons for main group elements alkali metals, alkali earth metals, haloge ...
... Review for exam 2 (Chapters 4 (all), 5 (all), 6 (6.1 to 6.3)) Chapter 4 The periodic table general organization of the table, rows (periods) and columns (groups) main group, transition metals, lanthanides, actinides valence electrons for main group elements alkali metals, alkali earth metals, haloge ...
Review for second exam:
... Review for exam 2 (Chapters 4 (all), 5 (all), 6 (6.1 to 6.3)) Chapter 4 The periodic table general organization of the table, rows (periods) and columns (groups) main group, transition metals, lanthanides, actinides valence electrons for main group elements alkali metals, alkali earth metals, haloge ...
... Review for exam 2 (Chapters 4 (all), 5 (all), 6 (6.1 to 6.3)) Chapter 4 The periodic table general organization of the table, rows (periods) and columns (groups) main group, transition metals, lanthanides, actinides valence electrons for main group elements alkali metals, alkali earth metals, haloge ...
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.