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Chemistry: Spring Semester Lecture Notes
... This is an unstable, momentary condition called the ____________________. e.g., When e– falls back to a lower-energy, more stable orbital (it might be the orbital it started out in, but it might not), atom releases the “right” amount of energy as… ...
... This is an unstable, momentary condition called the ____________________. e.g., When e– falls back to a lower-energy, more stable orbital (it might be the orbital it started out in, but it might not), atom releases the “right” amount of energy as… ...
Chemical Bonding
... • Going from left to right across a given period, the atomic number (no. of p) increases positive charge on the nucleus (nuclear charge) increases. • This means that there is a greater force of attraction for the electrons in the shell and the distance between the electrons and the nucleus decreas ...
... • Going from left to right across a given period, the atomic number (no. of p) increases positive charge on the nucleus (nuclear charge) increases. • This means that there is a greater force of attraction for the electrons in the shell and the distance between the electrons and the nucleus decreas ...
Atoms, Elements, and Ions
... What: Solid Sphere Model (1st atomic theory) •Elements are made up of indivisible particles called atoms •Each element was composed of the same kind of atoms. •Different elements were composed of different kinds of atoms. •Compounds are composed of atoms in specific ratios. •Atoms are not created or ...
... What: Solid Sphere Model (1st atomic theory) •Elements are made up of indivisible particles called atoms •Each element was composed of the same kind of atoms. •Different elements were composed of different kinds of atoms. •Compounds are composed of atoms in specific ratios. •Atoms are not created or ...
Lesson 6 What are the subatomic particles of an atom
... All pupils will be able to (Baseline): Recall what atomic number represents. Most pupils will be able to (Further): Describe the structure of the atom and why atoms have no overall charge. Some pupils will be able to (Challenge): Describe the trends in atomic radius down a group and across a period. ...
... All pupils will be able to (Baseline): Recall what atomic number represents. Most pupils will be able to (Further): Describe the structure of the atom and why atoms have no overall charge. Some pupils will be able to (Challenge): Describe the trends in atomic radius down a group and across a period. ...
atomic theory of matter
... the anionlike substance. – The more cationlike element appears to the left of or below the other element in the periodic table ...
... the anionlike substance. – The more cationlike element appears to the left of or below the other element in the periodic table ...
The format of this test is MULTIPLE CHOICE
... 1. __Condensation___ occurs when a gas becomes a liquid. 2. All matter is made up of tiny particles called __atoms___. 3. When a solid becomes a liquid, _melting_____ occurs. 4. An _element_____ is made up of only one type of atom. 5. __freezing___ changes a liquid into a solid. 6. A mixture is made ...
... 1. __Condensation___ occurs when a gas becomes a liquid. 2. All matter is made up of tiny particles called __atoms___. 3. When a solid becomes a liquid, _melting_____ occurs. 4. An _element_____ is made up of only one type of atom. 5. __freezing___ changes a liquid into a solid. 6. A mixture is made ...
Atomic History Timeline
... • Thought that all things were made of tiny, invisible, indestructible particles, called atoms • Thought atoms varied in size, shape and ...
... • Thought that all things were made of tiny, invisible, indestructible particles, called atoms • Thought atoms varied in size, shape and ...
Gateway Chemistry Review (Answer Key) Structure and Properties
... The atomic mass of each atom represents an average of all of the individual isotopes of that element. Two atoms contain the same number of protons but different numbers of neutrons. Isotopes are atoms of the same element, but have different masses. Isotopes with an unstable nucleus will tend ...
... The atomic mass of each atom represents an average of all of the individual isotopes of that element. Two atoms contain the same number of protons but different numbers of neutrons. Isotopes are atoms of the same element, but have different masses. Isotopes with an unstable nucleus will tend ...
Midterm Review Date
... A) Their metallic properties decrease and their atomic radii decrease. B) Their metallic properties decrease and their atomic radii increase. C) Their metallic properties increase and their atomic radii decrease. D) Their metallic properties increase and their atomic radii increase. 19. Which elemen ...
... A) Their metallic properties decrease and their atomic radii decrease. B) Their metallic properties decrease and their atomic radii increase. C) Their metallic properties increase and their atomic radii decrease. D) Their metallic properties increase and their atomic radii increase. 19. Which elemen ...
The format of this test is MULTIPLE CHOICE
... 1. __Condensation___ occurs when a gas becomes a liquid. 2. All matter is made up of tiny particles called __atoms___. 3. When a solid becomes a liquid, _melting_____ occurs. 4. An _element_____ is made up of only one type of atom. 5. __freezing___ changes a liquid into a solid. 6. A mixture is made ...
... 1. __Condensation___ occurs when a gas becomes a liquid. 2. All matter is made up of tiny particles called __atoms___. 3. When a solid becomes a liquid, _melting_____ occurs. 4. An _element_____ is made up of only one type of atom. 5. __freezing___ changes a liquid into a solid. 6. A mixture is made ...
Honors Mid-Term Review Sheet
... 57. What does each row on the periodic table represent? 58. How did Mendeleev arrange his periodic table? 59. How is the modern periodic table arranged? 60. What determines an element’s chemical properties? ...
... 57. What does each row on the periodic table represent? 58. How did Mendeleev arrange his periodic table? 59. How is the modern periodic table arranged? 60. What determines an element’s chemical properties? ...
8.1 Atoms and Their Parts Assignment
... number of protons and electrons are usually equal. This equality is important so that the atom as a whole is neither positively nor negatively charged. It is said to be neutral. Electrons have nearly 0 mass. Electrons orbit in specific locations starting closest to the nucleus. Two electrons fit in ...
... number of protons and electrons are usually equal. This equality is important so that the atom as a whole is neither positively nor negatively charged. It is said to be neutral. Electrons have nearly 0 mass. Electrons orbit in specific locations starting closest to the nucleus. Two electrons fit in ...
document
... ___T______20. The number of atoms on both sides of an equation must be equal for each element. Part C: For each of the following compounds, identify the number of atoms of each element. ...
... ___T______20. The number of atoms on both sides of an equation must be equal for each element. Part C: For each of the following compounds, identify the number of atoms of each element. ...
Name Date Class Period ______
... Name ______________________________________ Date __________________ Class Period _________ Atoms, Elements, and Compound Test Study Guide I. ...
... Name ______________________________________ Date __________________ Class Period _________ Atoms, Elements, and Compound Test Study Guide I. ...
John Dalton`s atomic theories were introduced in 18 hundreds
... however, he made a mistake in thinking atoms of element in a 1:1 ratio, and his system of atomic weights was not correct. He gave oxygen an atomic weight of seven instead of eight. The idea of atoms had been discovered much earlier. The Greeks had talked about atoms, but Dalton's theory was differen ...
... however, he made a mistake in thinking atoms of element in a 1:1 ratio, and his system of atomic weights was not correct. He gave oxygen an atomic weight of seven instead of eight. The idea of atoms had been discovered much earlier. The Greeks had talked about atoms, but Dalton's theory was differen ...
Unit 2: All Biology is Chemistry
... Isotopes are atoms of the same element that have different numbers of neutrons. – therefore they will have different mass numbers – this is the reason for the average atomic mass in the periodic table Click here to compare these twoare atoms. These two atoms both carbon atoms. But the atom on the le ...
... Isotopes are atoms of the same element that have different numbers of neutrons. – therefore they will have different mass numbers – this is the reason for the average atomic mass in the periodic table Click here to compare these twoare atoms. These two atoms both carbon atoms. But the atom on the le ...
Atomic Structure
... Definition : Isotopes are atoms of the same element with the same number of protons but different number of neutrons; Isotopes have the same atomic number but different mass numbers. ...
... Definition : Isotopes are atoms of the same element with the same number of protons but different number of neutrons; Isotopes have the same atomic number but different mass numbers. ...
Atoms, Molecules, and Ions (2)
... given chemical compound always has the same relative numbers and types of atoms. Chemical reactions involve reorganization of atoms—changes in the way they are bound together. The atoms themselves remain ...
... given chemical compound always has the same relative numbers and types of atoms. Chemical reactions involve reorganization of atoms—changes in the way they are bound together. The atoms themselves remain ...
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.