10/14 Chemistry Quiz

ENC and atomic size

smaller the atom is, harder for the elecrton to be removed (high ionization energy). Higher ENC is stronger/smaller atomic size that low ENC

oxidation state

the charge an element can form

The larger the atom is

the easier it is to remove an electron (low ionization energy)

first ionization energy

the energy required to remove the first electron from an atom -once occurred the atom has a charge -low ionization energy makes it easier to remove an electron -high is difficult

Period Law

the physical and chemical properties of the elements are periodic functions of their atomic numbers

atomic radius

the size of an atom- from nucleus to edge of electron cloud measured in angstrom- 1 x 10^10 Used to two to find radius because the cloud too faded to pick an end

cations

smaller that original because entire shell goes away during ionization

Which elements are correctly listed in order of INCREASING ionization energy? 1. O < F < Ne 2. O < S < Se 3. N < O < F 4. C < N < O 5. N < P < As

1. O < F < Ne

Which of the following elements would be expected to have the highest electronegativity? 1. P 2. Al 3. Ge 4. As 5. Li

1. P

Electronegativity values generally increase as you go across a row from left to right on the periodic table. 1. True 2. False

1. True

Henry Moseley

1913 Arranged the periodic table by atomic number instead of mass number

What is the correct order of increasing electronegativity for B, C, F, and Fr? 1. Fr, C, B, F 2. Fr, B, C, F 3. B, F, Fr, C 4. F, C, B, Fr 5. F, B, C, Fr

2. Fr, B, C, F

Which of the following would be expected to have the highest first ionization energy? 1. Li 2. O 3. Ne 4. F 5. C

3. Ne

Let X be a hypothetical element. Which of the following would be largest? 1. X + 2. X 3. X 2− 4. X 2+ 5. X −

3. X 2−

Which of the following would be most likely to form positive ions? 1. carbon (C) 2. fluorine (F) 3. lithium (Li) 4. sulfur (S)

3. lithium (Li)

Which of the following elements would be expected to have the highest electronegativity? 1. P 2. Na 3. Al 4. N 5. C 6. He

4. N

Which of the following elements would have the lowest first ionization energy? 1. Na 2. O 3. I 4. Rb 5. Cl

4. Rb

Which one of the following isoelectronic ions would be expected to have the largest radius? 1. Ca2+ 2. Cl− 3. K + 4. S 2− 5. Ga3+

4. S 2−

Which of the following would be expected to have the lowest first ionization energy? 1. C 2. Ne 3. O 4. F 5. Li

5. Li

Which of the following elements would be expected to have the highest first ionization potential? 1. K 2. Mn 3. P 4. S 5. O

5. O

Electronegativity

A measure of one atom's nuclei attraction for another atom's electron in a bond -scale from 0-4 -fluorine is most -n/a for Nobel gases (don't bond)

Be or Li- higher ionization energy

Be

Metals

Elements that are good conductors of electric current and heat, high density, malleable, strong, shiny, ductile, high melting/boiling point

Nonmetals

Elements that are poor conductors of heat and electric current, brittle, dull, low melting/boiling point

Metalloids

Elements that may have properties of both metals and nonmetals based on the conditions. -shiny but brittle -semi conductors

Which neutral atom has the smallest size? 1. O 2. F 3. Be 4. Li 5. B

F

diatomic elements

H2, N2, O2, F2, Cl2, Br2, I2 (bond to itself in nature)

Na or K- higher ionization energy

Na

increasing reactive order - K, Na, Rb, Cs

Na, K, Rb, Cs

Which of the following atoms would have the smallest size (atomic radius)? 1. Li 2. N 3. O 4. B 5. S

O

Dimitri Mendeleev

Russian scientist that created the periodic table according to atomic mass -accurate + able to predict missing elements and their properties

s-2 or K+ is bigger

S-2 (fewer protons)

Which has the larger atomic radius, S or Si?

Si

Most Reactive metals

are the largest because they are best electron givers

Most reactive nonmetals

are the smallest, best electron takers

polyatomic ions + examples

charged particles that are made of more than one atom Nitrate- (NO3)-1 Carbonate- (CO3)-2 Phosphate- (PO4)-3

Why down a group increases energy

each family step down, new levels added to electron cloud, making atom larger

electronegativity to atomic size for a period

increase in number, smaller the size, the higher the ENC, the greater pull (greater EN), nucleus closer to electrons (greater attraction)

When you move across a period, what does the ENC do

increases which pulls cloud closer, making atom smaller Calculated: ENC= Z(#p+) - S(shielding e-)

electronegativity to atomic size for a group

larger atomic size is, farther away (lower EN)

anions

larger than original electrons added to outer energy level (bigger based on electron-electron repulsion)