name: carla martinez valence electrons practice the valence electrons are the electrons in the outermost energy level. they are always the outermost electrons. atoms that lose electrons are called cations and have an overall positive charge. atoms that gain electrons are called anions and have an overall negative charge. determine the element’s number of valence electrons (# of electrons in the “outermost” shell). example: carbon has 4 valence electrons, carbon 4 1. fluorine 7 2. lithium 1 3. phosphorus 5 4. francium 1 5. calcium 2 6. carbon 4 7. nitrogen 5 8. iodine 7 9. silicon 4 10. oxygen 6 11. argon 8 12. barium 2 13. potassium 1 14. aluminum 3 15. helium 2 16. hydrogen 1 17. magnesium 2 18. xenon 8 19. sulfur 6 20. boron 3 21. bromine 7 22. what are valence electrons of an atom used for? 23. which groups on the periodic table want to lose electrons? what kind(s) of elements are these groups? 24. which groups on the periodic table want to gain electrons? what kind(s) of elements are these groups? 25. why do the elements from question 23 want to lose electrons? why do the elements from question 24 want to gain electrons? (hint: the answer is the same for both questions.). 26. how many valence electrons do the alkaline earth metals have? are these elements very reactive? explain your answer. 27. what is the name of the atoms that lose electrons? what is their overall charge? 28. what is the name of the atoms that gain electrons? what is their overall charge?

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### Question 22
# Brief Explanations:
Valence electrons are used in chemical bonding. Atoms interact (bond) with other atoms by transferring (ionic bonding) or sharing (covalent bonding) valence electrons to achieve a stable electron configuration (like a noble gas, usually 8 valence electrons, or 2 for hydrogen/helium).
# Answer:
Valence electrons are used for chemical bonding (to form compounds by transferring or sharing electrons to achieve a stable electron configuration like a noble gas).

### Question 23
# Brief Explanations:
Groups 1 (Alkali Metals), 2 (Alkaline Earth Metals), and 13 (some elements like Aluminum) on the periodic table tend to lose electrons. These are metals (alkali metals, alkaline earth metals, and some post - transition metals). Metals have low electronegativity and relatively few valence electrons (1, 2, or 3 for many), so losing electrons gets them to a stable electron configuration (like a noble gas).
# Answer:
Groups 1 (Alkali Metals), 2 (Alkaline Earth Metals), and 13 (e.g., Al) want to lose electrons. These groups contain metals (alkali metals, alkaline earth metals, and some post - transition metals).

### Question 24
# Brief Explanations:
Groups 15, 16, and 17 (Halogens) on the periodic table tend to gain electrons. Group 15 has 5 valence electrons, group 16 has 6, and group 17 has 7. These groups contain non - metals (and some metalloids in group 15). Non - metals have high electronegativity and need to gain electrons (1, 2, or 3 respectively) to achieve a stable octet (8 valence electrons, or 2 for hydrogen).
# Answer:
Groups 15, 16, and 17 want to gain electrons. These groups contain non - metals (and some metalloids in group 15).

### Question 25
# Brief Explanations:
Elements that want to lose electrons (from question 23) and those that want to gain electrons (from question 24) do so to achieve a stable electron configuration, specifically a noble gas electron configuration (usually 8 valence electrons, or 2 for hydrogen/helium). For example, a sodium atom (group 1) has 1 valence electron; losing it gives it the electron configuration of neon (a noble gas). A chlorine atom (group 17) has 7 valence electrons; gaining 1 gives it the electron configuration of argon (a noble gas).
# Answer:
Both groups want to achieve a stable noble gas electron configuration (having 8 valence electrons, or 2 for H/He). Elements that lose electrons do so to get rid of excess valence electrons to reach this stable state, and elements that gain electrons do so to fill their outer shell to reach this stable state.

### Question 26
# Brief Explanations:
Alkaline Earth metals are in group 2 of the periodic table. So they have 2 valence electrons. These elements are very reactive because they want to lose their 2 valence electrons to achieve a stable noble gas electron configuration (like the noble gas before them). Since they have a relatively low ionization energy (the energy required to remove an electron) compared to many other elements, they readily lose these 2 electrons in chemical reactions.
# Answer:
Alkaline Earth metals have 2 valence electrons. Yes, these elements are very reactive. They readily lose their 2 valence electrons to achieve a stable noble gas electron configuration, and they have relatively low ionization energy, so they react easily.

### Question 27
# Brief Explanations:
Atoms that lose electrons are called cations. When an atom loses electrons, it has more protons than electrons. Since protons are positively charged and electrons are negatively charged, the overall charge of the cation is positive. For example, a sodium atom (Na) loses 1 electron to become $Na^+$, which has a + 1 charge.
# Answer:
Atoms that lose electrons are called cations. Their overall charge is positive.

### Question 28
# Brief Explanations:
Atoms that gain electrons are called anions. When an atom gains electrons, it has more electrons than protons. Since electrons are negatively charged and protons are positively charged, the overall charge of the anion is negative. For example, a chlorine atom (Cl) gains 1 electron to become $Cl^-$, which has a - 1 charge.
# Answer:
Atoms that gain electrons are called anions. Their overall charge is negative.

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