Trending in the Periodic Table of Elements-Part 2

Multiple Choice

How is an atom related to matter?

• all matter is made up of atoms

• all atoms are made up of matter

• matter and atoms are NOT related

• matter and atoms are inversely related

Multiple Choice

He arranged the elements into groups that had similar properties allowing him to predict the properties and places in the chart of a yet undiscovered elements.

• John Dalton

• Niels Bohr

• Dmitri Mendeleev

• Henry Gwyn Jeffreys Moseley

Multiple Choice

What does the Periodic Law states?

• that when elements arranged in order of increasing ATOMIC NUMBER, their physical and chemical properties show a periodic pattern

• that when elements arranged in order of increasing ATOMIC MASS their physical and chemical properties show a periodic pattern

• that when elements arranged in order of increasing ATOMIC WEIGHT their physical and chemical properties show a periodic pattern

Fill in the Blanks

Multiple Choice

What is the atomic number?

• 58.693

• Ni

• Nickel

• 28

Multiple Choice

How many neutrons are there in this element?

• 79

• 118

• 196

• 275

Multiple Choice

What subatomic particle defines the identity of an element?

• electron

• neutron

• proton

Multiple Choice

Hydrogen has zero neutrons.

• True

• False

Multiple Choice

Using the periodic table of elements, identify the following elements if it is metal, nonmetal, metalloids.

1. Cl (17)

2. As (33)

3. Pb (82)

• 1. metal

  2. nonmetal

  3. metalloid

• 1. metalloid

  2. metal

  3. nonmetal

• 1. metalloid

  2. nonmetal

  3. metal

• 1. nonmetal

  2. metalloid

  3. metal

Fill in the Blanks

Fill in the Blanks

The elements in Group 1A are called Alkali Metals (except H), those in Group 2A are called Alkaline Earth Metals, the ones in Group 7A are called Halogens, and those in Group 8A are called noble gases.

​Sometimes, families are named after the first element: Group 3A is called the Boron Family, Group 5A Nitrogen Family and Group 6A Oxygen Family or Chalcogens.

​Periodic Trends: Atomic Size

​Atomic size decreases from left to right within a period. Atomic size increases from top to bottom.

​across-addition of proton and electron (distance is the same for e- and nucleus)

below-addition of proton and addition of electron (orbital)​ (distance increase for e- and nucleus)

​Atomic radius is the distance from the atoms nucleus to the outermost electron orbital

Multiple Choice

Arrange the following according to increasing atomic size.

Se, Br, Ga, Ca, K

• Br-K-Ca-Ga-Se

• Br-Se-Ga-Ca-K

• K-Ca-Ga-Se-Br

• Br-Ga-Ca-K-Se

​Periodic Trends: Electronegativity

Electronegativity increases from left to right. Electronegativity decreases from top to bottom.

Electronegativity is the ability of the atom to attract toward itself the electrons in a chemical bond.​

​across:

​high values of valence electron=high electronegativity

down:

closer distance of nucleus to the valence electron​=high electronegativity

Multiple Choice

Predict the element with higher electronegativity from each pair.

Cl or F

• Cl

• F

Multiple Choice

Predict the element with higher electronegativity from each pair.

C or O

• C

• O

​Ionization Energy- is the energy required to remove an electron from an atom.

Electron Affinity-is the amount of energy released or absorbed when an electron is added to an atom to form a negative ion.

​left to right =increases

​

bottom to top=increases​

​