Matter - Chapter 5.2 - 5.6

Question 1

Define Atom

Answer 1

The smallest particle of a chemical element that can exist.

Question 2

Define Cation

Answer 2

A positively charged ion

Question 3

Define Proton

Answer 3

A stable subatomic particle occurring in all atomic nuclei, with a positive electric charge.

Question 4

Define mass number

Answer 4

the total number of protons and neutrons in a nucleus.

Question 5

Define Valence shell

Answer 5

The valence shell is the outer shell of the atom

Question 6

Define Nobel gases

Answer 6

Any of the gaseous elements helium, neon, argon, krypton, xenon, and radon, occupying Group 0 (18) of the periodic table.

Question 7

Describe Rutherford’s and Bohr’s
models.

Answer 7

The Rutherford Model shows an atom with electrons orbiting a fixed, positively charged nucleus. The Bohr model shows electrons travel in defined circular orbits around the nucleus.

Question 8

Explain the difference between Mass Numbers & Atomic Numbers and be able to
correctly write the conventional representation of an element

Answer 8

While the mass number is the sum of the protons and neutrons in an atom, the atomic number is only the number of protons.

Question 9

Determine the number of protons, neutrons and electrons of an element based on Mass Number and Atomic Number.

Answer 9

Together, the number of protons and the number of neutrons determine an element’s mass number: mass number = protons + neutrons

Question 10

State the maximum number of electrons in electron shells.

Answer 10

The first shell holds 2 electrons. The second shell holds 8 electrons. The third shell holds 18 electrons. The fourth shell holds 32 electrons

Question 11

Using the periodic table what is the information shown on each of the periodic plates

Answer 11

At the top is the atomic number with the symbol in the middle and the electronic configuration at the bottom. With the atomic number at the top.

Question 12

Explain the differences between groups and periods in the periodic table

Answer 12

Elements in a group share similar chemical or physical properties. On the other hand, elements in the same period share the same electron configuration.

Question 13

Explain different emission spectrum by referring to the activity of electrons.

Answer 13

An emission spectrum consists of all the radiations emitted by atoms or molecules

Question 14

Explain why some ions are positively charged and
why others are negatively charged in relation to
their electrons.

Answer 14

Ions form when atoms gain or lose electrons. Since electrons are negatively charged, an atom that loses one or more electrons will become positively charged; an atom that gains one or more electrons becomes negatively charged