Elements and ATOMS
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The document discusses the structure of atoms and the properties of elements. It states that atoms are made up of subatomic particles, including protons, neutrons, and electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. The number of protons determines the element and is called the atomic number. Atoms can have different numbers of neutrons, forming isotopes of an element. The attraction between protons and electrons keeps the atom electrically neutral. The structure of atoms determines how elements react chemically.
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ATOM STRUCTURE AND PROPERTIES OF ELEMENTS
This document discusses the structure of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons, with the nucleus containing protons and neutrons at the center and electrons orbiting around it. The document also discusses isotopes, which are variants of the same element that differ in their number of neutrons. It notes that the number of protons determines an element's atomic number and properties. Finally, it explains that an atom's structure determines how it reacts chemically based on how tightly its electrons are held.
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Matter is composed of basic building blocks called atoms. Atoms were originally thought to be indivisible spheres, but are now understood to have internal structure. Atoms contain a tiny, dense nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, while neutrons and electrons can vary between atoms of the same element. Most atoms are electrically neutral, but can become ions by gaining or losing electrons.
atoms
This document provides an overview of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons determines the element, and the number of neutrons contributes to the mass number. The document also discusses the periodic table and how it can be used to find information about elements such as the number of protons, neutrons, and electrons. It includes some example calculations and provides additional online resources for learning more about atomic structure.
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Early chemists believed that all matter was composed of combinations of four elements - air, earth, fire and water. Later, it was discovered that all matter is composed of atoms, which are mostly empty space. Atoms contain electrons, protons and neutrons. Electrons orbit the nucleus in distinct energy levels. The number of protons determines the element. Chemical bonds form when atoms gain, lose or share electrons to achieve a full outer energy level. There are three main types of bonds - ionic, covalent and metallic. Chemical reactions occur when bonds are formed or broken.
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Atoms are the basic building blocks of all matter and consist of a small, dense nucleus surrounded by electrons. The nucleus contains protons and neutrons, with protons providing a positive charge and neutrons having no charge. Electrons orbit the nucleus and have a negative charge, keeping the overall atom electrically neutral. Atoms can vary in the number of neutrons while maintaining the same number of protons, creating different isotopes of an element. Radioactivity occurs when unstable atoms undergo nuclear decay and emit particles or energy.
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This document discusses the structure of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons, with the nucleus containing protons and neutrons at the center and electrons orbiting around it. The document also discusses isotopes, which are variants of the same element that differ in their number of neutrons. It notes that the number of protons determines an element's atomic number and properties. Finally, it explains that an atom's structure determines how it reacts chemically based on how tightly its electrons are held.
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This document provides an overview of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons determines the element, and the number of neutrons contributes to the mass number. The document also discusses the periodic table and how it can be used to find information about elements such as the number of protons, neutrons, and electrons. It includes some example calculations and provides additional online resources for learning more about atomic structure.
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1. The document discusses the atomic structure of matter, which is made up of protons, electrons, and neutrons. Atoms contain protons and neutrons in their nucleus, surrounded by electrons.
2. Atoms of different elements have different atomic structures because they contain different numbers of protons and electrons. Neutral atoms have equal numbers of protons and electrons, but atoms can gain or lose electrons to become ions.
3. The document then discusses subatomic particles like protons, neutrons, and electrons in more detail, including their relative masses and charges. It also discusses isotopes and how they have the same number of protons but different numbers of neutrons.
Atomic Structure Notes.pdf
Atoms are the basic building blocks of matter and are composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons occupy energy levels that orbit around the nucleus. The number of protons determines the element and is referred to as the atomic number. Atoms are electrically neutral overall, with the same number of protons and electrons, while neutrons have no charge. The mass number accounts for the total number of protons and neutrons in the atomic nucleus. Electrons can only occupy certain energy levels, with the first level holding up to two electrons and successive levels increasing in capacity.
Atomic Structure Isotopes
The document discusses atomic structure and isotopes. It recaps atomic structure, including the structure of the atom, relative masses and charges of protons, neutrons and electrons, chemical symbols, and electronic configuration. It then defines isotopes as atoms of the same element that contain the same number of protons but different numbers of neutrons. Examples of isotopes of oxygen are provided. Finally, some uses of radioactive isotopes are mentioned, such as in food irradiation, archaeological dating, smoke detectors, and as radioactive tracers.
Atomic structure chemistry review 11th
Atoms are made up of protons, neutrons, and electrons. The number of protons defines the element and is called the atomic number, while the total number of protons and neutrons is the mass number. Atoms are electrically neutral because they contain an equal number of protons and electrons, and isotopes are atoms of the same element that have different numbers of neutrons.
Atomic structure chemistry review 11th
Atoms are made up of protons, neutrons, and electrons. The number of protons defines the element and is called the atomic number, while the total number of protons and neutrons is the mass number. Atoms are electrically neutral because they contain an equal number of protons and electrons, and isotopes are atoms of the same element that have different numbers of neutrons.
Periodic table and elements along with a
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Atomicsstructure
- Atoms are the building blocks of matter and are made up of protons, neutrons, and electrons. The nucleus contains protons and neutrons and accounts for nearly all an atom's mass, while electrons orbit the nucleus.
- The number of protons determines the element and cannot be changed. Neutrons can vary between atoms of the same element, creating isotopes of that element.
- An atom's mass number is the total number of protons and neutrons, while its atomic mass refers to the average mass of all isotopes of that element as found in nature.
Structure of an Atom ppt cscope
Atoms are the building blocks of matter and consist of a nucleus surrounded by electrons. The nucleus contains protons and neutrons, and most of an atom's mass is in the nucleus. Electrons orbit the nucleus in energy levels. The number of protons determines the element and is an atom's atomic number. An atom's atomic mass comes from the total number of protons and neutrons.
Naresh
The periodic table arranges elements in order of increasing atomic number and groups elements with similar chemical properties together. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties. Atoms are made up of protons and neutrons in the nucleus and electrons in energy levels outside the nucleus. Atoms are neutral when they have an equal number of protons and electrons. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different atomic masses. An element's relative atomic mass takes into account the abundance of each isotope.
Naresh Periodic Table
The periodic table arranges elements in order of increasing atomic number and groups elements with similar chemical properties together. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties. Atoms are made up of protons and neutrons in the nucleus and electrons in energy levels outside the nucleus. Atoms are neutral when they have an equal number of protons and electrons. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different atomic masses. An element's relative atomic mass is averaged from the masses of its naturally occurring isotopes.
Atomic structure by uzair atif
Atoms are made up of subatomic particles including protons, neutrons, and electrons. Each element is defined by its number of protons, while isotopes of an element have different numbers of neutrons but the same number of protons. The relative atomic mass of an element is the ratio of the average mass of one of its atoms to 1/12 the mass of one carbon-12 atom. Electrons occupy shells around the nucleus, with the first shell holding up to 2 electrons and subsequent shells able to hold more electrons in a stable configuration.
Atomicstructure isotopes-100312015827-phpapp02
This document provides an overview of atomic structure and isotopes. It begins by recapping atomic structure, including the structure of the atom with electrons orbiting the nucleus, and the relative masses and charges of protons, neutrons, and electrons. It then defines isotopes as atoms of the same element with the same number of protons but different numbers of neutrons. Examples of different isotopes of oxygen are provided. The document concludes by discussing some uses of radioactive isotopes, such as in food irradiation and carbon dating.
Structure of atom (igcse)
1. Atoms consist of a positively charged nucleus surrounded by electrons that orbit in defined shells or energy levels.
2. The number of protons in the nucleus defines the atomic number of an element, while the total number of protons and neutrons gives the mass number.
3. Chemical properties are determined by valence electrons in the outer shell. Elements tend to gain or lose electrons to achieve a stable outer shell of 8 electrons.
Atoms
1) Atoms are the smallest units that make up matter and consist of protons, neutrons and electrons. Electrons orbit the nucleus in shells.
2) There are two main types of bonds between atoms - ionic bonds which involve transfer of electrons between metals and non-metals, and covalent bonds which involve sharing of electrons between non-metals.
3) Isotopes are atoms of the same element that have different numbers of neutrons, giving them different masses but the same chemical properties. Radioactive isotopes are unstable and decay over time.
Unit iii the atom and the prediodic table (2)
This document discusses the structure of atoms and the periodic table. It begins by introducing atomic theories proposed by scientists like Dalton, Thomson, Rutherford, Bohr and Schrodinger. It then discusses subatomic particles like protons, neutrons and electrons. The document explains how elements are organized on the periodic table based on their atomic number and electronic configuration. It provides examples of writing out electronic configurations and identifying protons, neutrons and electrons in different isotopes.
ATOMS.pptx
Atoms are the smallest particles that can exist independently and are made up of subatomic particles like protons, neutrons, and electrons. Atoms of the same element have the same number of protons but can differ in the number of neutrons forming isotopes. Chemical bonds like ionic bonds form when electrons are transferred, covalent bonds when electrons are shared, and metallic bonds by the flow of electrons in metal atoms. The periodic table organizes elements according to their atomic structure.
ATOMIC-STRUCTURE.pdf
Atoms are made up of three fundamental subatomic particles: protons, neutrons, and electrons. The atomic number of an element determines its identity and represents the number of protons in its nucleus. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same chemical properties. Electrons orbit the nucleus in shells at increasing distances from the nucleus. The number of electrons in the outer shell determines an element's chemical properties and reactivity.
Pwpt chemistrycin
The document discusses the composition and structure of matter at the atomic and molecular levels. It defines elements as pure substances that cannot be broken down chemically, and explains that atoms are the basic units that make up elements. Atoms contain protons and neutrons in the nucleus, and electrons in energy levels surrounding the nucleus. Elements combine to form compounds with unique properties. Compounds are represented by chemical formulas showing the elements and ratios present.
Pwpt chemistrycin
The document discusses the composition and structure of matter at the atomic and molecular levels. It defines elements as pure substances that cannot be broken down chemically, and explains that atoms are the simplest particles that make up elements. Atoms contain protons and neutrons in the nucleus, and electrons in energy levels surrounding the nucleus. Elements combine to form compounds with unique properties. Compounds are made of two or more elements bonded together in fixed proportions.
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Chapter 5
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Elements and ATOMS
- 1. ATOMS , THEIR STRUCTURE AND THE PROPERTIES OF ELEMENTS Miss Sofía Paz An element smallest posible piece…
- 2. First: Different elements or compounds have different properties: States (luquid, solid, gas, plasma) this properties depend on the atoms of the elements! MADE UP OF SUBATOMIC PARTICLES: -PROTONS(+) -NEUTRONS -ELECTRONS(-) ATOM: Smallest possible piece of an element (without loosing their properties)
- 3. The attraction of the negatively charged electrons and the positively charged protons keeps the electrons close to the nucleus.
- 4. How this subatomic particles form an ATOM? -NUCLEOUS: NEUTRONS, PROTONS(+), -CLOUD OF ELECTRONS (-) The attraction of the negatively charged electrons and the positively charged protons keeps the electrons close to the nucleus. Electrons have less mass than neutrons and protons.
- 5. NOT constantConstant ATOMIC NUMBER (Z)( NUMBER OF PROTONS) # of # of The number of protons is constant in each element The atom is electrically neutral, positive charges are balanced with the negative charges. NO two elements have the same atomic number the number of protons = the Atomic Number(Z)
- 6. ISOTOPES (when the number of neutrons change) Alternate forms of elements (always same proton number but different neutron number) Why C14, C13, C12??? Is the NUCLEAR NUMBER: NUMBER OF PROTONS + NUMBER OF NEUTRONS
- 7. RADIOACTIVE ISOTOPE: HOMEWORK FOR NEX CLASS! What are radioactive isotopes and What uses does they have? CONCEPT :CHEMICAL PROPERTIES ARE BASED ON STRUCTURE OF ATOMS
- 8. ElECTRONS AND REACTIVITY: Electrons properties: -amount of energy -how thigly they are held by protons Depending on this properties electrons belong to differents energy leves: I energy level can hold up to 2 electrons II energy level can hold up to 8 electrons III energy level can hold up to 18 electrons HOW DOES ATOMS STRUCTURE DETERMINE HOW IT REACTS??
- 10. CONCEPT :CHEMICAL PROPERTIES ARE BASED ON STRUCTURE OF ATOMS I energy level :2 electrons II energy level: 8 electrons III energy level : 18 electrons
- 11. ATOM SONG! 3.21 MIN https://www.youtube.com/watch?v=O5iaw5WNuB 0
- 12. CONCEPT :CHEMICAL PROPERTIES ARE BASED ON STRUCTURE OF ATOMS Element/ isotope Atomic Number Protons Neutrons Total electrons (same number ofprotons+) Electrons in the highest level 12C 6 14C 14N 7 16O 8 P 15 15 S 16 16
- 13. Just howsmall is an atom?? http://www.youtube.com/watch?v=yQP4UJhNn0I DOGS TEACHING CHEMSITRY http://www.youtube.com/watch?v=addK0b2Isw8
- 14. Element/ isotope Atomic Number Protons Neutrons Total electrons (same number of protons) Electrons in the highest level 12C 6 6 6 6 4 14C 6 6 8 6 4 14N 7 7 7 7 5 16O 8 8 8 8 6 P 15 15 15 15 5 S 16 16 16 16 6