Periodic Trends Graphing Activity
Part 1: Group Trends
Group 1:
Group 7:
Part 2: Period Trends
Period 3:
General Periodic Table:
1. State the periodic law in your own words.
Chemical and physical properties of elements repeat in each period when elements are arranged in order of atomic mass
2. How do the properties analyzed in this activity show periodicity of the chemical elements? That is, as the atomic number increases, when do the trends repeat?
For the most part, the trend carried out throughout the period. However there were some cases when Argon, a noble gas did not follow a trend and another case where the trend was interrupted due to the
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What is electronegativity?
Electronegativity measures the ability of an atom to attract a bonding pair of electrons.
16. What is the most electronegative element and where is it found on the periodic table? (Top, bottom, left, right?)
Fluorine is the most electronegative element; it is a halogen and is found in the upper right corner of the periodic table.
17. Where are the least electronegative elements found? (Top, bottom, left, right?)
The least electronegative elements are found towards the bottom left of the periodic table (the opposite corner of fluorine)
18. What appears to be the trend in electronegativity as you move from left to right in a row?
Electronegativity increases as we move from left to right
19. What appears to be the trend in electronegativity as you move from top to bottom in a column?
Electronegativity decreases as we move from up to down
20. List the following atoms in order of increasing electronegativity: O, Al, Ca
Ca, Al, O
21. List the following atoms in order of decreasing electronegativity: Cl, K, Cu
Cl, Cu, K
Ionization Energy:
26. Define Ionization
Question # 1: Part A How many electrons and protons in an atom of vanadium? Answer # 1: Atomic number = number of protons = 23 Mass number = number of protons + neutrons Mass number = 51 g/mole Number of neutrons = 51-23 Number of Neutrons = 28 Number of electrons = atomic number = 23 Question
4.) I noticed that there is a relationship between the ionic radius and the atomic number of the representative elements in Group 1A. The higher the atomic number, the bigger the ionic radius is. So, while hydrogen has an atomic number of 1 and Francium has an atomic number of 87, it is safe to assume that FR has a higher ionic radius. This is true; the ionic radius for Hydrogen is 0.012, and for Francium, it is 0.194.
According to the Bohr model of hydrogen atom, the kinetic and potential energies of the electrons vary as .......... .. and... distance of electron from the nucleus. respectively. where r is the The square of the wavefunction, y}, gives us the Absorption of a given amount of energy gives rise to a larger increase in entropy the the initial temperature. Orbital energies in multi-electron atoms are mere difficult to calculate due to the additional Select the correct answers from the following multiple choice questions.
Task 1 (P1) The periodic table is laid out into groups and periods. They are also put into different blocks S-Block, D-Block, P-block and F-Block due to their energy levels. They are organised by their energy levels and chemicals properties. As the elements go along the periods in the periodic table the electronegativity increases but as the elements go down the groups the electronegativity decreases.
Our latest lab covered a detailed description of atoms and molecules, laid out in a distinctive way using balls and sticks for valence electrons and bonds. We were given charts to fill out recoding our findings regarding several molecules and their electron count, type of bonds,
One must look to see which element has both violet and orange spectra lines. It is shown that the element Cesium is the only element that has both violet and orange spectra lines. 2. Describe two different approaches to exciting the electrons that exist in elements. Offer a specific reason why scientists use different approaches to excite the electrons of different elements.
Where as, electrons are negatively charged(Doc.3).The neutron is the dense middle of the atom(Doc.3). The protons and neutrons in the atom are in the nucleus(Doc.3). However, the electrons preside in electron clouds outside the nucleus(Doc.3). To sum up, an atom is a small structure that defines what an element is and
The trend decreases going down a group because the atom is
As atoms go down a family, they become more metallic. Since they are becoming more metallic, the atoms want to lose electrons and therefore don’t hold the electrons as tightly, also making the atom larger. Typically as elements go across a series, they decrease in
If more number of vacant ‘d’ orbitals are present then there may be difficulty for dehydrogenation process because gases are strongly chemisorbed. VIII group elements contain one e- in their vacant ‘d’ orbital. This is called electronic factor of elements. Second condition is metal atoms should have spaced and ordered arrangement.
Although not linear, a trend that is established is that as one looks across a period there is an increase in density until around group 11 in period IV. This trend varies depending on the row being examined but for the most part has an increase, an area of consistency, then a decrease. This trend can be observed based on the graph comparing Period IV density and atomic number. The point of decrease occurs around atomic number 28.
P1 - Volumetric Analysis Made Easy The periodic table is split into 8 different categories. Group 1 consists of alkali metals which are very reactive. However group 7 contains very reactive non-metals. The periodic table starts from alkali and ends at noble gases (Group 8).
Meyer stated if each element is arranged in order of their atomic weights, and fall into groups of similar chemical and physical properties. If the atomic weights were plotted as ordinates and the atomic volumes as abscissae, the curve obtained a series of maxima and minima. The most electropositive elements appear at the peak of curve in order of their atomic weights. One contribute Meyer had was the concept that carbon atoms in benzene were arranged in a ring. Except, he didn’t propose the alternation of single and double bonds, that was included later in a structure by August
Protons are positively charged, neutrons are not charged and electrons are negatively charged. The proton and the neutron are stuck together, that is called nuclei, and the electron orbits the nucleus in a wave like motion. The amount of protons, neutrons, and electrons can change, creating different atoms with different energy levels.
The ions occupying the A and B lattice sites are detailed in Fig. (1.1). Figure 1.1: Schematic of compositions ABO 3 [1]. The perovskite structure is versatile and robust.