Matter, Chemical Trends and Chemical Bonding Test

Question 1

Names, symbols and electrical charges of the three subatomic particles

Answer 1

Protons: P+
Neutrons: N^0
Electrons: e-

Question 2

Where is basically all the mass of an atom? What contributes to this mass?

Answer 2

Protons and neutrons account for most of an atom’s mass. These subatomic particles are found in the nucleus of the atom

Question 3

Defines the terms atomic number and mass number

Answer 3

Mass number- Total number of protons and neutrons

Atomic number -# of protons or electron

Question 4

What is it called when an atom gains an electron?

Answer 4

Negative ion also known as anion

Question 5

What is it called when an atom looses an electron?

Answer 5

Positive ion also known as a cation

Question 6

What is a period? Group/family?

Answer 6

• Horizontal rows of elements called periods.

- The vertical columns of elements are called groups/families

Question 7

Which is an alkali metal? Ca, Cu, In, Li, S

Answer 7

LITHIUM

Question 8

Which is a halogen? Ce, Hg, Si, O, I

Answer 8

IODINE

Question 9

Which is a transition element? Pb, W, Ca, Cs, P

Answer 9

TUNGSTEN, LEAD

Question 10

Which is a noble gas? Xe, Se, H, Sr, Zr

Answer 10

XENON

Question 11

What is an isotope? Does calcium have more or less than 20 neutrons? Explain

Answer 11

Isotopes are atoms of elements with different numbers of neutrons. Calcium has 20 neutrons (atomic mass-atomic#)

Question 12

Sample of 100 Mg atoms, 55 were Mg-24, 25 were Mg-25 and 20 were Mg-26. According to the data, what is the average atomic mass? Why does it not perfectly match whats on the periodic table

Answer 12

The average atomic mass is going to be more near 24 because it is the most common out of the 3. The reason why it doesn’t perfectly match what’s on the periodic table is because it incorporates the other averages into the equation.

Question 13

Describe the trend in atomic sizes on the periodic table.

Answer 13

Atomic size decreases from left to right across a period of elements and increases down a group.

Question 14

Define ionization energy

Answer 14

Energy required to remove the valence electron

Question 15

IE trends

Answer 15

Ionization energy increases from left to right

Question 16

Difference between ionization energy and electron affinity

Answer 16

Ionization energy: the energy required to remove an electron from a neutral atom.
Electron affinity: the energy change when a neutral atom attracts an electron to become a negative ion

Question 17

Do metals or non metals have a higher ionization energy?

Answer 17

non-metals

Question 18

Define electronegativity

Answer 18

Tendency of an atom to attract a bonding pair of electrons

Question 19

Decribe trends in electronegativity on the periodic table

Answer 19

Down a group- decreases

Left to right across a period- increases

Question 20

Which atom has the highest electronegativity

Answer 20

Fluorine

Question 21

Why do noble gases have no measured electronegativity value

Answer 21

Noble gases already have their full outer valence shell of electrons, they don’t want to grab electrons at all

Question 22

Diatomic molecules

Answer 22

HOFBrINCl

Question 23

Physical properties of a compound

Answer 23

Color, odor, melting point and boiling point