Section 1: Introduction to Atoms

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section 1 Introduction to Atoms

Presentation transcript:

Section 1: Introduction to Atoms How did atomic theory develop and change? What is the modern model of the atom?

Atomic Theory and Models Dalton thought that atoms were like smooth, hard balls that could not be broken into smaller pieces.

Atomic Theory and Models Thomson suggested that atoms had negatively charged electrons embedded in a positive sphere.

Rutherford’s Gold Foil Experiment Rutherford was surprised that a few particles were deflected strongly. This led him to propose an atomic model with a positively charged nucleus.

Later Atomic Models Through the first part of the twentieth century, atomic models continued to change.

Modern Model of an Atom This model of a carbon atom consists of positively charged protons and neutral neutrons in a nucleus that is surrounded by a cloud of negatively charged electrons.

Particles in an Atom An atom is composed of positively charged protons, neutral neutrons, and negatively charged electrons. Protons and neutrons are about equal in mass. An electron has about 1/2,000 the mass of a proton or neutron.

Isotopes Atoms of all isotopes of carbon contain six protons and six electrons, but they differ in their number of neutrons. Carbon-12 is the most common isotope.

More on Atomic Structure Click the PHSchool.com button for an activity about atomic structure.

End of Section: Introduction to Atoms