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elements
and
chemical
bonds
Atoms Bond
Elements rarely exist in pure form in nature.
Instead, atoms of different elements chemically
combine and form compounds.
H
X
H20
✓
Atoms Bond
Compounds make up most of the matter around
you, including living and nonliving things.
H20
C02
02
C6H12O6
positions of Electrons
• The exact position of the
electrons in an atom cannot
be determined. Electrons
constantly move around the
nucleus.
• However, each electron is
usually in a certain area
around the nucleus. Some are
in areas close to the nucleus
and some are in areas farther
away.
Electrons and energy
• The areas in which electrons move around the nucleus are
called energy levels.
Electrons and energy
• Different electrons in an atom
have different amounts of
energy.
• The amount of energy an
electron has is related to its
distance from the nucleus.
• Electrons closest to the
nucleus are in the lowest
energy level. These electrons
have the least energy.
• Electrons farthest from the
nucleus are in the highest
energy level.
Electrons and energy
• The lowest energy level in the atom can hold only two
electrons.
• The second energy level can hold up to eight electrons.
Electrons and bonding
• Like magnets, the negatively charged electrons are
attracted to the positively charged nucleus of an atom.
• Electrons close to the nucleus have a strong attraction
to it.
Nail A
Nail B
Which has the stronger
attraction to the magnet?
valence electrons
• Electrons farthest from their nucleus are easily
attracted to the nuclei of nearby atoms.
valence electrons
• These outermost electrons are the only electrons
that form chemical bonds.
valence electrons
• A valence electron is an outermost electron of an atom
that participates in chemical bonding. Valence
electrons have the most energy of all the electrons in
an atom.
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 1 has 1 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 2 has 2 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 13 has 3 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 14 has 4 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 15 has 5 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 16 has 6 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 17 has 7 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Group 18 has 8 valence electron
valence electrons
• The number of valence electrons in an atom helps
determine the type and number of bonds the atom
can form.
• The periodic table can tell you the number of valence
electrons an atom has.
Except for helium, which has 2.
electron dot diagram
• An electron dot diagram is a simple way to show an
element’s valence electrons.
• An electron dot diagram is a model that represents
valence electrons in an atom as dots around the
element’s chemical symbol.
ClN
5 valence electrons 7 valence electrons
electron dot diagram
• Electron dot diagrams can help you predict how an
atom will bond with other atoms.
ClN
5 valence electrons 7 valence electrons
electron dot diagram
electron dot diagram
electron dot diagram
electron dot diagram
electron dot diagram
• Notice that a neon atom, Ne,
has eight valence electrons. It
has no unpaired dots.
• Atoms with eight valence
electrons are chemically stable.
They do not react easily with
other atoms.
• Atoms with 1–7 valence
electrons are chemically
unstable. These atoms easily
bond with other atoms and
form compounds.
noble gases
• The elements in Group 18 are called noble gases. With
the exception of helium, noble gases have eight
valence electrons and are chemically stable.
• Stable atoms do not easily react, or form bonds, with
other atoms.
Ar
stable and unstable atoms
• Atoms with unpaired dots in their electron dot
diagrams are reactive, or chemically unstable.
• Nitrogen, for example, is reactive because it has three
unpaired dots.
• Unstable atoms such as nitrogen become more stable
by forming chemical bonds with other atoms.
N
stable and unstable atoms
• When an atom forms a bond, it gains, loses, or shares
valence electrons with other atoms.
• By forming bonds, atoms become more chemically
stable.
• Atoms are most stable with eight valence electrons.
Therefore, atoms with less than eight valence
electrons form bonds and become stable.
N

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Elements and Chemical Bonds

  • 2. Atoms Bond Elements rarely exist in pure form in nature. Instead, atoms of different elements chemically combine and form compounds. H X H20 ✓
  • 3. Atoms Bond Compounds make up most of the matter around you, including living and nonliving things. H20 C02 02 C6H12O6
  • 4. positions of Electrons • The exact position of the electrons in an atom cannot be determined. Electrons constantly move around the nucleus. • However, each electron is usually in a certain area around the nucleus. Some are in areas close to the nucleus and some are in areas farther away.
  • 5. Electrons and energy • The areas in which electrons move around the nucleus are called energy levels.
  • 6. Electrons and energy • Different electrons in an atom have different amounts of energy. • The amount of energy an electron has is related to its distance from the nucleus. • Electrons closest to the nucleus are in the lowest energy level. These electrons have the least energy. • Electrons farthest from the nucleus are in the highest energy level.
  • 7. Electrons and energy • The lowest energy level in the atom can hold only two electrons. • The second energy level can hold up to eight electrons.
  • 8. Electrons and bonding • Like magnets, the negatively charged electrons are attracted to the positively charged nucleus of an atom. • Electrons close to the nucleus have a strong attraction to it. Nail A Nail B Which has the stronger attraction to the magnet?
  • 9. valence electrons • Electrons farthest from their nucleus are easily attracted to the nuclei of nearby atoms.
  • 10. valence electrons • These outermost electrons are the only electrons that form chemical bonds.
  • 11. valence electrons • A valence electron is an outermost electron of an atom that participates in chemical bonding. Valence electrons have the most energy of all the electrons in an atom.
  • 12. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has.
  • 13. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 1 has 1 valence electron
  • 14. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 2 has 2 valence electron
  • 15. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 13 has 3 valence electron
  • 16. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 14 has 4 valence electron
  • 17. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 15 has 5 valence electron
  • 18. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 16 has 6 valence electron
  • 19. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 17 has 7 valence electron
  • 20. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Group 18 has 8 valence electron
  • 21. valence electrons • The number of valence electrons in an atom helps determine the type and number of bonds the atom can form. • The periodic table can tell you the number of valence electrons an atom has. Except for helium, which has 2.
  • 22. electron dot diagram • An electron dot diagram is a simple way to show an element’s valence electrons. • An electron dot diagram is a model that represents valence electrons in an atom as dots around the element’s chemical symbol. ClN 5 valence electrons 7 valence electrons
  • 23. electron dot diagram • Electron dot diagrams can help you predict how an atom will bond with other atoms. ClN 5 valence electrons 7 valence electrons
  • 28. electron dot diagram • Notice that a neon atom, Ne, has eight valence electrons. It has no unpaired dots. • Atoms with eight valence electrons are chemically stable. They do not react easily with other atoms. • Atoms with 1–7 valence electrons are chemically unstable. These atoms easily bond with other atoms and form compounds.
  • 29. noble gases • The elements in Group 18 are called noble gases. With the exception of helium, noble gases have eight valence electrons and are chemically stable. • Stable atoms do not easily react, or form bonds, with other atoms. Ar
  • 30. stable and unstable atoms • Atoms with unpaired dots in their electron dot diagrams are reactive, or chemically unstable. • Nitrogen, for example, is reactive because it has three unpaired dots. • Unstable atoms such as nitrogen become more stable by forming chemical bonds with other atoms. N
  • 31. stable and unstable atoms • When an atom forms a bond, it gains, loses, or shares valence electrons with other atoms. • By forming bonds, atoms become more chemically stable. • Atoms are most stable with eight valence electrons. Therefore, atoms with less than eight valence electrons form bonds and become stable. N