Metals and Nonmetals
List one property of metals.
Shiny
Malleable
Ductile
Electrically Conductive
Thermally Conductive
Who has the bigger atomic size?
Mg vs. Na
Which has the higher first ionization energy? Na or Cl?
Cl
What is a chemical bond?
The attractive force that keeps two atoms together.
What happens to atomic radius as you go down a group?
It gets bigger.
List one property of nonmetals
Poor conductor of heat
Poor conductor of electricity
Brittle
Why does atomic size increase as you go down a group?
The number of electron shells increases.
Why does ionization energy increase across a period?
Effective nuclear charge increases.
Which has higher electronegativity, metals or nonmetals?
Nonmetals
What happens to ionization energy as you move left to right across a period?
It increases.
In metals, electrons are __________ (tightly/loosely) bound to atoms.
In nonmetals, electrons are __________ (tightly/loosely) bound to atoms.
Tightly
Why does atomic size decreases as you move left to right across a period?
Effective nuclear charge increases.
Rank Li, Na, K, and Cs in order of ionization energy, from least to greatest.
1) Cs
2) K
3) Na
4) Li
What type of bond forms between a metal and nonmetal?
Ionic
Which element has the higher electronegativity: O or F?
F
Why are metals good conductors of electricity?
Their electrons are loosely bound, which allows for electron movement and current to flow.
If the internuclear distance between two nitrogen atoms is 110 pm, what is the atomic radius?
65 pm
Define ionization energy.
The energy required to remove a valence electron from an atom.
Is the H-Cl bond ionic or covalent? Explain why.
Nonmetal + Nonmetal
A student claims that potassium (K) has higher ionization energy than lithium (Li). Explain why the student is incorrect.
Ionization energy is greater when the number of electron shells is smaller. Lithium has less electron shells than potassium, so it must have greater ionization energy.
Provide an example of a molecule that has a covalent bond.
1) NaCl
2) O2
Explain the role of effective nuclear charge in determining atomic size.
Effective nuclear charge is the net positive charge valence electrons in an atom experience. A greater effective nuclear charge means stronger binding of outermost electrons, which leads to a smaller radius.
Which element has the higher first ionization energy, O or S. Explain your reasoning using periodic trends.
O has a higher ionization energy.
O has less electron shells than S, which leads to a higher ionization energy.
Define electronegativity.
The force that the positive nucleus of an atom exerts on valence electrons of another atom.
Explain why electronegativity increases as you move up a group.
The number of electron shells increases, which means that atoms can get closer to each other. This increases the electric force exerted by the positive nucleus onto the other atom's valence electrons.