Chemistry Flashcards
(46 cards)
What happens to nonmetal reactivity as you move across a period (left to right)?
Decreases → Metals on the left lose electrons easily, but as you move right, atoms hold onto electrons more tightly.
Why does atomic radius decrease across a period from left to right?
The number of protons increases, strengthening the nuclear pull on electrons, pulling them closer to the nucleus.
Why does atomic radius increase down a group?
More electron shells are added, making the atom larger.
What is ionization energy?
The amount of energy required to remove an electron from an atom.
Why does ionization energy increase across a period?
More protons increase nuclear attraction, making it harder to remove an electron.
What is electronegativity?
An atom’s ability to attract electrons in a bond.
Why does electronegativity decrease down a group?
Larger atomic radius weakens the nuclear attraction for electrons.
Why does electronegativity increase across a period?
More protons strengthen nuclear attraction, pulling bonding electrons closer.
Why do alkali metals (Group 1) react violently with water?
They have one valence electron, which they lose easily, forming highly reactive compounds.
Why are alkaline earth metals (Group 2) less reactive than alkali metals?
They have two valence electrons, requiring more energy to remove both.
Why do halogens (Group 17) have high electronegativity?
They are small atoms with strong nuclear pull and only need one electron to complete their octet.
Why are noble gases (Group 18) unreactive?
Their valence shells are full, meaning they don’t need to gain or lose electrons.
Why do transition metals have multiple oxidation states?
They can lose different numbers of electrons due to their d-orbitals, leading to multiple charge states.
What are Lanthanides & Actinides, and why are they unique? and what are their characteristics?
They have incomplete f-orbitals, leading to special magnetic and optical properties.
How does metal reactivity change down a group?
Larger atomic radius = weaker nuclear hold = easier to lose electrons → more reactive.
How does nonmetal reactivity change across a period?
Increases → More protons = stronger pull on electrons, making it easier to gain them.
How does nonmetal reactivity change down a group?
Decreases → Larger atomic radius = weaker attraction for electrons = harder to gain them.
Why are halogens (Group 17) the most reactive nonmetals?
They only need one electron to complete their octet, making them highly reactive.
What role does electronegativity play in nonmetal reactivity?
Nonmetals gain electrons, so high electronegativity means stronger reactivity.
Why do nonmetals prefer covalent bonding instead of losing electrons?
They have high electronegativity, so instead of losing electrons, they share them in covalent bonds.
What is an ionic bond?
An ionic bond is a chemical bond formed when a metal loses electrons and a nonmetal gains electrons, creating charged ions that attract each other.
What type of elements form ionic bonds?
Metals and nonmetals form ionic bonds because metals lose electrons easily while nonmetals gain electrons.
What structure do ionic compounds form?
Ionic compounds form a crystalline lattice, a repeating 3D pattern of ions that maximizes attraction and minimizes repulsion.
How does electronegativity affect ionic bonds?
Higher electronegativity in nonmetals allows them to steal electrons from metals, creating strong ionic attractions.
