KEY Chapter 4-2 Review Atoms, Isotopes and Ions

Complete the diagram of an atom below with these terms; nucleus, proton, neutron, electron, 1st energy level, 2nd energy level. The electrons are located in the _electron cloud_ _ .

Properties of Subatomic Particles (pg 109)particle Symbol Relative charge Relative mass (atomic mass units or amu)proton P+ +1 1neutron n 0 1Electron e- -1 0

Definitions

Atomic mass- average mass of all the isotpes of an element

Atomic number- number of protons in the nucleus

Mass number- neutrons + protons in the nucleus

Atom- smallest particle of an element

Isotope- atoms of a given element that have different numbers of neutrons and different mass numbers.

Ion- an atom or isotope that has positive or negative charge

Questions

proton

2nd energy level

nucleus

1st energy level

electron

neutron

1. List the charge and location of protons, neutrons and electrons in an atom.

protons positive one, Nucleus Elecrons- negative one, -1, in electron cloud

neutrons no charge, nucleus2. List the relative mass of protons, neutrons and electrons in an atom. Relative mass means the mass compared to

the other particles.

Protons, neutrons 1 atomic mass unit (amu),

electrons have a mass of 0 amu

3. Label this “symbol square” with these words; net charge, mass number, and atomic number, symbol of ele

How many electrons fit in each energy level?

first – 2 maximumsecond – 8 maximumthird - 18 maximum

5. Describe how to calculate the number of protons and neutrons in an atom using the atomic number and the mass number.

Protons = atomic numberNeutrons: mass number – atomic number (larger number – smaller number in “symbol square”)

6. Describe how to calculate the number of electrons from the net (overall) charge.Protons – electrons = net charge

7. Describe the similarity between each atom and its isotope.

Same # OF PROTONS, But different # of neutrons & different mass numbers

8. What pattern do you see with the subatomic particles (protons, neutrons, and electrons) in each of the ions that you created?

Protons ≠ electronsProtons & neutrons unchanged

KEY Neutral Atom (stable form) Isotope (stable form) Ion (stable form)

Net Charge

Atomic numberOr number of protons

Mass number

Symbol of element H - hydrogen

2) name _____________ p+ = 2 n= 1 e - 2

none none

3) name _____________ p+ = _____ n= _____ e - ______

p+ = ____ n = _____e - _____

p+ = ____ n = _____e - _____

4) name _____________ p+ = _____ n= _____ e - ______

p+ = ____ n = _____e - _____

Unstable

p+ = ____ n = _____e - _____

5) name _____________ p+ = _____ n= _____ e - ______ p+ = ____ n = _____e - _____

p+ = ____ n = _____e - _____

7

Neutral Atom (stable form) Isotope (stable form) Ion (stable form)

6) name _____________ p+ = _____ n= _____ e - ______

p+ = ____ n = _____e - _____

p+ = ____ n = _____e - _____

7) name ____________ p+ = _____ n= _____ e - ______

p+ = ____ n = _____e - _____

p+ = ____ n = 7e - 10

8) name _____________ p+ = _____ n= _____ e - ______ p+ = ____ n = _____e - _____

p+ = ____ n = _____e - _____

11

-4

-3

17

9) name _____________ p+ = _____ n= _____ e - ______

p+ = ____ n = _____e - _____

NONE

p+ = ____ n = _____e - _____

10) name ___________ p+ = _____ n= _____ e - ______

p+ = ____ n = _____e - _____

p+ = ____ n = _____e - _____

Describe the pattern in the way that the electrons are organized on the atoms. You may use your textbook for help.

16

First energy level filled w/2 electrons; second energy level filled with 8 electrons

What pattern do you see with the subatomic particles (protons, neutrons, and electrons) in each of the neutral atoms that you created?

Protons = electrons Protons + neutrons = mass number