Grade 10 and 11 Science Chapter 1 review

A toms and elements

1 what is an atom?

• An atom is the smallest particle of matter. It cannot be divided chemically (p. 7).

• Because atoms are too small to be examined directly, scientists have devised various models to represent them (p. 7).

• According to Dalton, the atom is like a billiard ball—solid and indivisible. All the atoms of a single element are identical (same mass, same size, same chemical properties), but different from those of other elements (p. 8).

• The electron is one of the particles that make up an atom. It is negatively charged (p. 11).

• The proton is one of the particles that make up an atom. It is found in the nucleus and carries a positive charge (p. 13).

• The Rutherford-Bohr atomic model is a representation of the atom as a very small nucleus made up of positively charged protons, surrounded by negatively charged electrons moving in defined orbits (p. 15).

2 THE PERIODIC CLASSIFICATION OF THE ELEMENTS

• A periodic classification is a way to group the elements according to certain properties (p. 17).

• The periodic table of the elements is a visual presentation of the elements in groups according to their physical and chemical properties (p. 17).

• The elements can be classified into three categories: metals, nonmetals and metalloids (p. 20).

• A valence electron is an electron in the outermost shell of an atom (p. 21).

• A group corresponds to a column of the periodic table. The elements in a particular group have similar chemical properties because they all have the same number of valence electrons (p. 21).

• A period corresponds to a row of the periodic table. All the elements in a period have the same number of electron shells (p. 23).

3 REPRESENTING ATOMS

• The information needed to represent an atom is provided in the periodic table (p. 27).

• Lewis notation is a simplified representation of the atom, in which only the valence electrons are illustrated. They are placed one by one around the symbol, like the four points on a compass. When these four positions are filled, the electrons are then doubled to form pairs (p. 27).

• In the Rutherford-Bohr model, a small, positively charged nucleus is represented by a small ball containing the atomic number of the element and a “+” sign (symbolizing the protons). The ball is surrounded by as many circles as there are electron shells in the atom (the number of shells equals the period number). The valence electrons (smaller balls containing a “–” sign) are placed on the outermost electron shell in a pattern similar to Lewis notation (like the four points on a compass). The remaining electrons needed to reach the atomic number are added to complete the inner electron shells (pp. 27–28).

• As its name suggests, in the “ball-and-stick” model, the atom is depicted as a ball whose size is generally proportional to the number of electron shells. The bonds connecting it to other atoms are represented by sticks (p. 29).