Chapter 4: Problem 53
Which elements would you expect to lose electrons in chemical changes? (a) potassium (b) sulfur (c) fluorine (d) barium (e) copper
Short Answer
Expert verified
Elements likely to lose electrons in chemical changes are (a) potassium, (d) barium, and (e) copper, as these are metals.
Step by step solution
01
Understand Electron Transfer in Chemical Changes
In chemical changes, elements tend to lose or gain electrons to achieve a more stable electron configuration. Generally, metals are more likely to lose electrons and become cations, while non-metals are more likely to gain electrons and become anions. This is related to their position in the periodic table.
02
Identify the Position in the Periodic Table
Identify whether each element is a metal or a non-metal. Metals, which are generally found on the left side and the center of the periodic table, tend to lose electrons. Non-metals, found on the right side of the periodic table, tend to gain electrons.
03
Predict Electron Loss
Using the periodic table, predict which elements are likely to lose electrons: (a) Potassium (K) is an alkali metal and will lose electrons. (b) Sulfur (S) is a non-metal and is more likely to gain electrons. (c) Fluorine (F) is a halogen non-metal and is more likely to gain electrons. (d) Barium (Ba) is an alkaline earth metal and will lose electrons. (e) Copper (Cu) is a transition metal and will lose electrons.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Periodic Table
The periodic table is a tabular arrangement of the chemical elements, organized by increasing atomic number, electron configurations, and recurring chemical properties. Elements are placed into categories such as metals, non-metals, and metalloids. Metals, which occupy the left and middle portions of the table, are typically characterized by their ability to conduct electricity and heat, their malleability, and their tendency to lose electrons during chemical reactions, becoming positively charged ions, or cations. This trend is due to their lower electronegativity and the desire to reach a stable electron configuration by giving up electrons. On the right side, non-metals are more likely to gain electrons to form anions, with higher electronegativity allowing them to attract and hold onto electrons more easily.
Cation and Anion Formation
The formation of cations and anions is a fundamental process in chemistry, involving the transfer of electrons between atoms. Cations are positively charged ions that are created when an atom, typically a metal, loses one or more electrons. Losing electrons allows an atom to achieve a full outer shell, resembling the nearest noble gas in terms of electronic configuration, leading to a more stable and energetically favorable state.
Conversely, anions are negatively charged ions created when an atom, generally a non-metal, gains electrons. These extra electrons provide the non-metal atom with a full outer shell, thus stabilizing it. The ability of an element to lose or gain electrons is intrinsic to its position on the periodic table and is predictive of how it will behave in chemical reactions.
Conversely, anions are negatively charged ions created when an atom, generally a non-metal, gains electrons. These extra electrons provide the non-metal atom with a full outer shell, thus stabilizing it. The ability of an element to lose or gain electrons is intrinsic to its position on the periodic table and is predictive of how it will behave in chemical reactions.
Alkali Metals
Alkali metals, located in group 1 of the periodic table, are known for being highly reactive due to having a single valence electron that they can easily lose to form cations with a +1 charge. Elements like lithium (Li), sodium (Na), and potassium (K) are all members of this group.
Distinct Properties of Alkali Metals:
- They are soft and can be cut with a knife.
- They have low densities and melting points relative to other metals.
- Their reactivity increases as you move down the group.
- They react vigorously with water, producing hydrogen gas and alkaline hydroxides.
Alkaline Earth Metals
Alkaline earth metals form group 2 of the periodic table and include elements such as beryllium (Be), magnesium (Mg), calcium (Ca), and barium (Ba). These metals have two valence electrons and are less reactive than alkali metals but still lose their electrons relatively easily to form +2 charged cations.
Characteristics of Alkaline Earth Metals:
- They are harder, denser, and have higher melting points than alkali metals.
- They are also reactive, although not as much as alkali metals, and tend to form oxides and hydroxides with water.
- The reactivity of alkaline earth metals also increases with the atomic number within the group.
Transition Metals
Transition metals consist of the elements found in groups 3 through 12 of the periodic table. They include both familiar metals such as iron (Fe), copper (Cu), and gold (Au), as well as less commonly known elements like hafnium (Hf) and tantalum (Ta).
Salient Features of Transition Metals:
- They exhibit variable oxidation states, often forming more than one type of cation.
- Transition metals are known for their ability to form complex ions, which are central to their catalytic activity in various chemical reactions.
- They have high melting points, high densities, and are usually very hard.
- Many transition metals are also capable of conducting electricity and heat efficiently.