This document provides an overview of atomic structure and chemical bonding. It discusses the following key points:
- About 25 elements are essential for life, with carbon, oxygen, hydrogen, and nitrogen making up 96% of living matter.
- Atoms are composed of protons, neutrons, and electrons. Chemical behavior is determined by the atom's electron configuration.
- Atoms combine via covalent bonds, which involve sharing electrons, and ionic bonds, which involve electron transfer. Weak bonds like hydrogen bonds also play important roles in biology.
- Covalent bonds form molecules, while ionic bonds form crystalline ionic compounds. Bond type depends on differences in electronegativity between atoms.
A presentation on atomic structure and chemical bond. Here you can find the full details of atomic structure and 5 types of chemical bond. This is for the course of Inorganic Pharmacy, Course code is PHAR-1103. This can be also used for Biochemistry students and other.
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#be like boss
Explains the structure of the atom and its discovery
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
A presentation on atomic structure and chemical bond. Here you can find the full details of atomic structure and 5 types of chemical bond. This is for the course of Inorganic Pharmacy, Course code is PHAR-1103. This can be also used for Biochemistry students and other.
Thank you. Like, Commen, Share
#be like boss
Explains the structure of the atom and its discovery
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
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Applied Chemistry, atomic and molecular structure, part 1, by Shiraz mahbob PhDMaqsoodAhmadKhan5
applied chemistry lecture and slide,
Applied Chemistry, atomic and molecular structure, part 1, by Shiraz mahbob PhD, lecturer in chemistry in pakistan institute of engineering and applied sciences
A nearly-comprehensive list of vocabulary terms needed for introductory chemistry in grade 9 science, including a variety of source websites for reference.
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https://arxiv.org/abs/2306.08302
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https://www.microsoft.com/en-us/research/blog/graphrag-unlocking-llm-discovery-on-narrative-private-data/
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The discussion will extend to how AI can be used to transform XML content. In particular, the focus will be on the use of AI XPath extension functions in XSLT, Schematron, Schematron Quick Fixes, or for XML content refactoring.
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9. • While all atoms of a given element have
the same number of protons, they may
differ in the number of neutrons.
• Two atoms of the same element that
differ in the number of neutrons are
called isotopes.
• In nature, an element occurs as a
mixture of isotopes.
– For example, 99% of carbon atoms have 6
neutrons (12
C).
– Most of the remaining 1% of carbon atoms
have 7 neutrons (13
C) while the rarest
isotope, with 8 neutrons is 14
C.
13. • Electrons have potential energy because of
their position relative to the nucleus.
– The negatively charged electrons are attracted
to the positively charged nucleus.
– The farther electrons are from the nucleus, the
more potential energy they have.
• However, electrons cannot occupy just any
location away from the nucleus.
• Changes in potential energy can only occur
in steps of a fixed amount, moving the
electron to a fixed location.
– An electron cannot exist between these fixed
locations.
18. • The first electron shell can hold only 2
electrons.
– The two electrons of Helium fill the first shell.
• Atoms with more than two electrons must
place the extra electrons in higher shells.
– For example, Lithium with three electrons has
two in the first shell and one in the second
shell.
• The second shell can hold up to 8
electrons.
– Neon, with 10 total electrons, has two in the
first shell and eight in the second, filling both
shells.
32. • An ionic bond can form if two atoms are
so unequal in their attraction for valence
electrons that one atom strips an electron
completely from the other.
– For example, sodium with one valence electron
in its third shell transfers this electron to
chlorine with 7 valence electrons in its third
shell.
– Now, sodium has a full valence shell (the
second) and chlorine has a full valence shell
(the third).
Fig. 2.14
38. • Hydrogen bonds form when a hydrogen
atom that is already covalently bonded to a
strongly electronegative atom is attracted to
another strongly electronegative atom.
– These strongly electronegative atoms are
typically nitrogen or oxygen.
– Typically, these bonds result because the polar
covalent bond with hydrogen leaves the
hydrogen atom with a partial positive charge
and the other atom with a partial negative
charge.
– The partially positive charged hydrogen atom is
attracted to negatively charged (partial or full)
molecules, atoms, or even regions of the same
large molecule.
48. • For example, we can recombine the covalent
bonds of H2 and O2 to form the new bonds of
H2O.
• In this reaction, two molecules of H2 combine
with one molecule of O2 to form two
molecules of H2O.
• The ratios of molecules are indicated by
coefficients.