Metallic character
What does metallic character refer to in terms of an element's electron behavior?
Metallic character refers to the tendency of an element to lose electrons and form cations.
The higher the ________ , the greater the non-metallic character
Electron affinity
How are Group 1 metals stored to prevent reactions with water?
They are stored in oil to prevent contact with water and avoid reactions.
Does the reactivity of alkali metals (Group 1) increase or decrease as you move down the group?
Answer: Increase
Explanation: As you move down Group 1, the reactivity increases because the atomic radius increases, and the outermost electron is more easily lost due to lower ionization energy.
Halogens have a tendency to _______ electrons.
Gain electrons
Where in the periodic table would you find elements with the greatest metallic character, and why?
Elements with the greatest metallic character are found towards the bottom left of the periodic table because they have lower ionization energies and a greater tendency to lose electrons.
What does electron affinity refer to?
Change in energy when neutral gas atom gains one electron to form a negative ion (anion)
What products are formed when Group 1 metals react with water, and why is hydrogen gas released?
When Group 1 metals react with water, they form metal hydroxides and release hydrogen gas. The reaction involves the metal losing an electron to water, resulting in the formation of hydroxide ions and hydrogen gas.
Do halogens (Group 17) become more or less reactive as you move down the group?
Answer Scheme:
Answer: Less reactive
Explanation: The reactivity of halogens decreases down the group because their atomic radius increases, and their ability to attract electrons (electronegativity) decreases.
Displacement reaction only occurs when _______ is stronger than _______.
Halogen, halide ion
Why does metallic character increase as you move down a group in the periodic table?
Metallic character increases down a group because atomic size increases, reducing ionization energy and making it easier for elements to lose electrons.
Name two factors that contribute to an element having high non-metallic character.
high electronegativity and high electron affinity
Why are Group 1 metals like sodium and potassium highly reactive with water, making them unsuitable for solid materials?
Group 1 metals are highly reactive with water because they readily lose their outer electron to form positive ions, which leads to reactions that produce heat, hydrogen gas, and hydroxides. This makes them unstable and unsuitable for use as solid materials.
Does the ionization energy of alkali metals increase or decrease as you move down the group?
Answer Scheme:
Answer: Decrease
Explanation: Ionization energy decreases as you move down Group 1 because the outer electron is farther from the nucleus and more shielded by inner electrons, making it easier to remove.
Do halogens (Group 17) react with halide ions to form new halogen compounds?
Answer Scheme:
Answer: Yes
Explanation: Halogens can react with halide ions to displace the halide from a compound if the halogen is more reactive than the halide. For example, chlorine can displace bromide ions from potassium bromide.
How does ionization energy relate to the metallic character of an element?
Ionization energy is the amount of energy required to remove an electron from a neutral atom. Elements with lower ionization energy have a greater tendency to lose electrons, which gives them greater metallic character.
Explain why non-metallic character decreases as you move down a group in the periodic table.
Because the atomic size increases, reducing the nucleus' attraction for valence electrons
How does the presence of water in the atmosphere affect the use of Group 1 metals in solid form?
Since water is present in the atmosphere, Group 1 metals react with it, which would cause them to break down and release hydrogen gas. This makes it impractical to use these metals in solid form for construction or as material surfaces without reactions occurring.
Which is more reactive: fluorine (F) or iodine (I)?
Answer Scheme:
Answer: Fluorine (F)
Explanation: Fluorine is more reactive than iodine because it has a smaller atomic radius and higher electronegativity, which allows it to attract electrons more easily during reactions.
In a displacement reaction between a halogen and a halide ion, does the more reactive halogen displace the less reactive halide ion?
Answer Scheme:
Answer: Yes
Explanation: In a displacement reaction, a more reactive halogen (like chlorine) will displace a less reactive halide ion (like bromide or iodide) from its compound. This is a classic redox reaction where the halogen gains an electron, and the halide ion loses one.
Why do elements with lower ionization energy have greater metallic character?
Elements with lower ionization energy require less energy to lose electrons, making it easier for them to form positive ions and exhibit stronger metallic character.
How does high electron affinity relate to an atom’s ability to gain electrons?
High electron affinity means the atom releases more energy when gaining an electron, showing a strong attraction for additional electrons.
How does the reactivity of Group 1 metals change down the group, and why does this happen?
The reactivity of Group 1 metals increases as you move down the group because ionization energy decreases. This makes it easier for these metals to lose their outermost electron, increasing their tendency to react with water and other substances.
When an alkali metal reacts with a halogen, does the alkali metal form a cation or an anion?
Answer Scheme:
Answer: Cation
Explanation: Alkali metals lose their single valence electron when they react with halogens, forming positively charged cations (e.g., Na⁺, K⁺). The halogen gains an electron to form a negatively charged anion (e.g., Cl⁻, I⁻).
What is the trend in reactivity between halogens and halide ions, and how does it explain the halogen displacement order (Cl₂ > Br₂ > I₂)?
Answer Scheme:
Answer: The reactivity of halogens decreases as you go down the group (Cl₂ > Br₂ > I₂).
Explanation: The reactivity of halogens decreases as you go down Group 17 because the atomic radius increases, and the electronegativity decreases, making it harder for larger halogens like iodine to gain electrons. Thus, chlorine, being the most reactive, can displace bromide and iodide ions from solutions, while iodine cannot displace bromine or chlorine.