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200 400 600 1000 200 400 600 800 1000 Bond-not James Periodic Trends Charged UP! Potpourri ANYTHING GOES! 1000 800
Bonding that occurs when electrons are given or taken away from an atom to form a compound. What is ionic? 1-200
Elements that SHARE electrons create this bond type. What is a covalent bond? 1-400
Which family of elements on the periodic table forms no stable compounds? What are Noble Gases? 1-600
One of the following compounds is not possible. N 2, KO, CO 2,CaO What is KO? 1-1000
Sugar has slight dipoles, causing it to dissolve in water but not conduct a charge. It forms this type of bond. What is POLAR covalent?
Electronegativity INCREASES as you go in this general direction on the periodic table. What is up and to the right?
Ionization energy DECREASES as you move in this general direction on the periodic table. What is down and to the left?
The ability to “attract” electrons to an atom is known as this. What is electronegativity?
How tightly an atom holds on to its electrons or the energy needed to remove electrons from protons is called this. What is Ionization Energy?
This element has THE highest electronegativity on the periodic table. What is Fluorine?
This happens when objects with LIKE electrical charges are brought together. What is REPEL?
This happens when objects with OPPOSITE electrical charges are brought together. What is attract?
The particle in the nucleus of an atom with no charge. What is a neutron?
A charged particle that has lost or gained electrons. What is an ion?
Metals are generally known for being good at this. What is conducting a charge?
Developed the FIRST theory of atoms. Who was Democritus? 4-200
Developed an atomic model involving electrons in specific energy levels? Who was Niels Bohr? 4-400
The metal ions we tested for the flame test produced different colored flames for this reason. What is electrons jumping and falling between energy levels? 4-600
Discovered that atoms contain a positive nucleus and are mostly empty space. Who was Ernest Rutherford? 4-800
In Niels Bohr’s experiment, he determined that the black spaces ON AN EMISSION SPECTRA represented this. What is areas where no electrons can orbit. 4-1000
To become happy and stable magnesium must… What is “lose two electrons”? 5-200
The reason F and Cl act very much the same in reactivity. What is same number of valence electrons/they’re in same column. 5-400
The dissolving of ionic substances into ions without the need for added energy. What is dissociation? 5-600
This is needed to remove an electron from a proton in a neutral atom. What is ionization energy? 5-800
This pair of elements (metal and non-metal) has the highest negativity difference on the periodic table. What is Fr and F? 5-1000
Elemental! Periodic Trends Charged UP! Potpourri ANYTHING GOES!
Bonding Periodic Table Potpourri Scientists ANYTHING GOES! 1000.
Chapter 16 Atomic Structure and Chemical Bonds. Why Do Atoms Combine???
Ionic Bonds LEARNING TARGET: HOW DOES AN ION BECOME POSITIVELY OR NEGATIVELY CHARGED? HOW DOES AN IONIC BOND FORM?
Valence electrons: Electrons in the highest energy level These electrons are the ones that bond!! The group A # matches how many valence electrons.
Periodic Trends. Types of Periodic Trends How elements differ as you move through the periodic table? Atomic Radius Ionic Radius Ionization Energy Electronegativity.
Atomic Structure & Chemical Bonds. A. The nucleus (containing protons & neutrons) is at the center of an atom and is surrounded by the electron cloud.
Periodic Properties Chemical and physical properties of the elements change with their position in the periodic table.
Chapter 6 Atomic Structure and Chemical Bonds. I. Atomic Structure At the center of every atom is a nucleus containing protons and neutrons Electrons.
1. How are the noble gases different from other groups of elements? a. Their atoms do not react easily with other atoms. b. They are nonmetals. c. They.
Electron Configuration and Periodic Properties/Trends Chapter 5 Section 3 Pgs
Unit 7 Changes in matter Chapter 19 Molecules and compounds.
Objectives Be able to explain why atoms sometimes join to form bonds Be able to explain why atoms sometimes join to form bonds Be able to explain why.
Ch. 7: Ionic Compounds & Metals Sec. 7.1: Ion Formation.
Periodic Table Trends and Similarities. Trends of the Periodic Table: At the conclusion of our time together, you should be able to: 1. Give a trend across.
What would you find in the nucleus of an atom? An electron has what charge? What is an element? Define matter: What does the atomic number correspond.
CHAPTER 2 COMPOSITION OF MATTER MATTER- anything that occupies space and has mass MASS- quantity of matter an object has ELEMENT- a pure substance that.
4 – Investigate and describe the compounds formed by bonding elements. 3 – Describe why certain elements bond with others. 2 – Use the periodic table.
Periodic Trends. Atomic Radius Defined as half of the distance between two bonding atoms nuclei.
Chemical Bonding. Chemical Bond A force that holds two or more atoms together ◦ This happens because atoms prefer to have a full outer shell ◦ Atoms can.
III. Periodic Trends. Types of Periodic Trends Atomic size (atomic radius) Ionic size (ionic radius) Ionization energy electronegativity.
Properties of Matter. Element A pure substance that cannot be broken down into simpler substances by ordinary chemical means. Sulfur.
Unit 9 Chapter 6 – Chemical Bonds. Essential Questions 1)What is the difference between compounds and mixtures? 2)Explain the difference between an ion.
I II III Periodic Trends. Valence Electrons Electrons available to be lost, gained, or shared in the formation of chemical compounds Outer energy.
Ionic & Covalent Bonds. A compound is a substance whose smallest unit is made up of atoms of more than one element bonded together.
Atomic structure and chemical bonds. Warm up – Nov 4 What are the subatomic particles, their location in the atom and their charges?
CH2 Sec1 Matter and Substances. Everything is made up of matter. Matter is anything that has mass and takes up space.
Periodic Trends Section 6.3 Objectives: AOD C.3.1 Define atomic radii, ionization energy, electronegativity, and energy levels. AOD C.3.2 Recognize periodic.
BONDS How does an ionic bond form? How does a covalent bond form? How does a metallic bond form? What are the properties of ionic and covalent compounds?
6.1 Ionic Bonding. Stable Electron Configurations When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not.
Periodicity E.Q.: What information can be obtained from the periodic table and how is it used?
Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.
Warm up What part of the atom has a positive charge and where is it found?
What you’ve learned so far….. Atoms form bonds in more than one way In IONIC bonding, atoms give up or gain electrons In COVALENT bonding, atoms.
Periodic Table Trends. Arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column,
Define these words Ion Ionic bond Ionic compound Chemical formula Subscript Covalent bond.
Trends in the Periodic Table. The rows are called periods (7) The columns are called groups (18)
The structure of an atom Atoms are the building blocks of matter. Atoms are made up of smaller particles: Protons are positively charged particles.
Matter- anything that has mass and occupies space Atom- basic unit of matter Subatomic particles: Protons (+) –in nucleus, 1 amu Neutrons (0) –in nucleus,
Bell Ringer 1. How many valence electrons does N have? 2. Which of the 3 “classes” on the periodic table displays properties of both metals and nonmetals?
Chapter 1 Chemical Bonding. All matter is made up of atoms. Atoms are the basic building blocks of all the substances in the universe.
Atomic Radius The radius of an atom. The radius of an atom. Periods - decreases as you move left to right across the table Periods - decreases as you move.
AIM: DETERMINING IONIZATION ENERGY AND ELECTRONEGATIVITY OF ELEMENTS DO NOW: 1. LIST IN ORDER OF INCREASING ATOMIC RADII: MAGNESIUM, SILICON, BARIUM, BROMINE.
Electrons are located in an area around the nucleus called the electron cloud. The electron cloud is made up of different energy levels. The electrons.
Matter is composed of tiny particles called atoms. Section 1: Atoms, Elements, and Compounds K What I Know W What I Want to Find Out L What I Learned.
Trends of the Periodic Table I. Oxidation Numbers (p. 222) II. Reactivity III. Atomic Radius (pp ) IV. Ionization Energy (pp ) V. Electronegativity.
Periodic Trends Each horizontal row is called a period because it corresponds to one full cycle of a trendEach horizontal row is called a period because.
Ionic and Covalent Compounds. How many valence electrons do atoms need in the highest energy level to be stable? 8.
NO WHOT WEEK Warm Up: With your desk partner (1 page for both) 1.On scratch paper, draw an atom, label its parts 2.Then… name 5 physical properties 3.Then.
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